Transcript Balancing Chemical Equations
Slide 1
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
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BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 2
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
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BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 3
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 4
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 5
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 6
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 7
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 8
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 9
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 2
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 3
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 4
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 5
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 6
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 7
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 8
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn
Slide 9
BALANCING CHEMICAL
EQUATIONS
USEFUL TERMINOLOGIES
• Chemical formula: It gives the information about
atoms or ions present in the chemical compound.
• Chemical equation: It is a symbolic representation of
reactants (present in left hand side in the chemical
reaction) and the products (present in right hand side
in the chemical reaction).
• Reactant --------- Products
• Chemical reaction: The process which leads to the
transformation of one set of chemical substances to
the other set of chemical substances.
• The Law of Conservation of Mass states that matter
cannot be created nor destroyed, only changed. The
mass of all of the reactants must equal the mass of all
the products. Chemical equations are balanced in
order to satisfy the Law of Conservation of Mass
LETS BALANCE
• The equation is said to balanced if it satisfies
the following conditions
• i)The number of atoms should be same on
reactant and product side.
• ii) The coefficients should be an integer.
• iii) The coefficients should have smallest
possible denominator.
• Some Rules for balancing equations:
• Use coefficients in front of formulas to balance equations
• DO NOT change a formula in order to balance an element
(DO NOT change subscripts).
• DO NOT add terms (atoms or formulas) to the equation
• Begin balancing with an element that occurs only one time
on each side of the arrow.
• Try to balance the elements one at a time (starting from left
to right)
• If the same polyatomic ion is seen on both sides of the ,
balance poly atomics (not the elements)
• Save for last:
• Elements appearing in more than two formulas
• Uncombined elements (an element all by itself)
• DO NOT use a coefficient of “1”; it is implied
• Check you work. Suggestion: use a tally system below the
equation.
• If the equation is balanced at the start, write the word
“balanced” at the end of the equation.
LETS TRY AN EXAMPLE
• Example 1 :
_____Na(s)
+____Cl2(g)
_____NaCl(s)
• The number of Na atoms to the left of the arrow=1 and the
number of Na atoms to the right =1
• The number of Cl atoms on the left -1 and number to the right of
the arrow 2
• Without balancing the equation, it looks like an atom of Cl has
been destroyed! This is impossible according to the Law of
Conservation of Mass.
• The equation must be balanced so that no atoms/mass is/are lost.
• If you place a 2 in front of the NaCl, this will give you 2 Na and 2 Cl
atoms to the right of the arrow
• Coefficient applies to all elements in the formula that follows
it; coefficient multiplies the subscript
• 2 NaCl means two units of NaCl
• Now, place a 2 in front of the Na.
• Is the equation balanced?
• Do the number of Na atoms and the number of Cl atoms on
the left of the arrow equal the number of Na atoms and Cl
atoms to the right of the arrow? Yes, therefore the equation is
balanced.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
BALANCING A WORDED EQUATION
Step 1: Iron reacts with oxygen to form ferric oxide.
Step 2: If we write the chemical equation in words
Iron + Oxygen -> Ferric oxide
Step 3: Now we balance the chemical equation
Fe + O2 Fe2O3
On left hand side 1 atom of Fe and 2 atoms of O and On right hand
side
2 atoms of Fe and 3 atoms of O
Here the equation is not balanced.
To balance the above equation
First we balance the oxygen atoms, multiply O2 with 3 in left hand side
and multiply Fe2O3
With 2, then
Fe + 3 O2 2 Fe2O3
In this equation 6 oxygen atoms are present on both sides. i.e., oxygen
atoms are balanced.
Now to balance the iron atoms Fe is multiplied with 4 on left hand
side, then
4 Fe + 3 O2 ->2 Fe2O3
Its Balanced Equation now.
ONE MORE …
• Step 1: Methane burns with Oxygen to form Carbon dioxide
and water molecule
• Step 2: If we write the chemical equation in words,
• Methane + Oxygen Carbon dioxide + water
• Step 3: Now we balance the chemical equation
• CH4 + O2 -> CO2 + H2O
• On left hand side 1 carbon atom, 4 atoms of H,2 atoms of
Oxygen and On right hand side we have 1 carbon atom, 3
atoms of oxygen and 2 hydrogen atoms
• Here the equation is not balanced. But the number of
carbon atoms on both sides is same. So now we balance
the remaining hydrogen and oxygen atoms in the above
equation.
• First balance the hydrogen atoms, for this purpose multiply
H2O with 2, then
• CH4 + O2 ---> CO2 + 2 H2O
• Now the number of oxygens are not equal on both sides. So
oxygen is multiply with 2 on left hand side, then we get
• CH4 + 2 O2 ---> CO2 + 2 H2O
WRITE THE CHEMICAL EQUATION FOR THE FOLLOWING
CHEMICAL REACTION AND THEN BALANCE IT.
• 1. Liquid water and calcium metal react to produce
aqueous calcium hydroxide and hydrogen gas.
• 2. Solid aluminum oxide decomposes to produce
aluminum metal and oxygen gas.
• 3. Sodium iodide reacts with lead (II) nitrate to produce
sodium nitrate and lead (II) iodide.
• 4. Ethane gas, C2H6, combines chemically with
atmospheric oxygen in a combustion reaction to produce
carbon dioxide gas and water vapor.
• 5. The aqueous solutions of lead (II) nitrate and potassium
sulfate react to form lead (II) sulfate solid and potassium
nitrate.
•
PRACTICE QUESTIONS
• 1. __NaCl + __BeF2 --> __NaF + __BeCl2
• 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4
• 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3
• 4. __CH4 + __O2 --> __CO2 + __H2O
• 5. __Mg + __Mn2O3 --> __MgO + __Mn