Transcript Slide 1

Coach Hyde
Physical Science Unit 5
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• The Law of Conservation of Matter:
states that for any system closed to all transfers
of matter and energy (both of which have mass),
the mass of the system must remain constant over
time, as system mass cannot change quantity if it is
not added or removed
• Soooo….. Matter cannot be created nor destroyed
it can only change form
• (this is the basic principle of all conservation laws
such as energy, matter, mass etc…
• Thank you Sir Antoine Lavoisier
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Something to discuss before we get started
• (s): Solid stated of matter
• (l): Liquid State of matter
• (g): gaseous State of Matter
• (aq): compound is in aqueous
solution with H2O
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Reactants = The starting substances (things that react)
Products
the
= The final substances (produced) after
reaction
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Exothermic Reaction: occurs when the
temperature of a system increases due to the evolution
of heat. This heat is released into the surroundings,
A system of reactants that absorbs heat from the
surroundings in an Endothermic Reaction.
How do you think this can be noticed/determined?
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If a chemical equation does not obey the law of
conservation of mass the equation is said to be what?
NOT BALANCED
So Let’s look at the steps we need to take to
BALANCE chemical equations
Let’s work with the following equation:
Fe +
O2

Fe2O3
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Step 1. Create a RAP table
(what’s a RAP table ??)
A table that shows us what atoms are present in this
reaction, how many there are and are they reactants
or products?
For example:
#R atom #P
1
2
Fe
O
2
3
Fe +
O2

Fe2O3
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Rule 2. Go to the first atom that’s not balanced and
balance it!
Since Fe atoms are not balanced what do we need to
do to balance it?
Right! Multiply it by 2 (Only multiply)
#R atom #P
2x 1
2
Fe
O
2
3
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In step 2 we balanced the number of Fe atoms by
multiplying the reactant side by 2. This now becomes
the new coefficient in the chemical equation.
#R atom #P
2x 1
2
Fe
O
2
3
Modify the equation to reflect the change
2Fe +
O2

Fe2O3
Are all atoms balanced?
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3. Move to the next unbalanced atom. What is it?
#R atom #P
2
2
Fe
O
2
3
How can we balance the
Oxygen?
Multiply Reactants by 3 and Products by 2
#R atom #P
2
3x2
Fe
O
2
3x2
Adjust the equation to reflect your
changes
2Fe +
3O2  2Fe2O3
But notice that by changing Oxygen we also
Changed Iron. We need to go back and fix this.
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4. Write out the updated RAP table. How can we
Balance the Iron?
#R atom #P
2x 2
6
Fe
O
4
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Sure! Multiply the # of
Reactant Fe atoms by 2 !
Re-write the equation reflecting
The new changes you’ve made.
4Fe +
3O2  2Fe2O3
Do we have a balanced Chemical Equation now?
Yes we do!
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Polyatomics
When an equation has Polyatomics in it, such as in this
Balanced chemical equation
2AgNO3 + MgCl2  2AgCl + Mg(NO3)2
And the polyatomic appears on BOTH the reactant and product
Side of the equation Count the polyatomic as an “ATOM”
So the above reactant atoms would be:
#R atom #P
If the same polyatomic does not
Appear on both sides break the
Polyatomic down into atoms!
2
2
1
2
Ag
NO3
Mg
Cl
2
2
1
2
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Is this equation balanced?
NaOH + CaBr2  Ca(OH)2 + NaBr
What atoms do we have in
This equation?
1) Count atoms & Start
the RAP table
#R atom #P
1
1
1
2
NA
OH
Ca
Br
1
2
1
1
2) Do the #Reactant atoms = the # of Product atoms?
3) So pick the 1st unbalanced atom & begin balancing
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We’ll start with balancing Hydroxide
NaOH + CaBr2  Ca(OH)2 +NaBr
How can we make both Hydroxides equal?
Sure we’ll multiply #R OH by 2
#R atom #P
1
Next step> rewrite the modified eqn. 2x 1
1
2NaOH + CaBr2  Ca(OH)2 + NaBr
2
Na
OH
Ca
Br
1
2
1
1
Hydroxide is now balanced so let’s move to the next
Unbalanced atom, which is? …
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What can we do to balance the Bromine?
Sure! Multiply the #P Bromine by 2
Now adjust the table to reflect
#R atom #P
The changes and then rewrite the
2
Na
1
Eqn.
2
OH 2
1
Ca
1
2
Br 1 x2
2NaOH + CaBr2  Ca(OH)2 + 2NaBr
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Let’s update the RAP table with the new #’s
Based on our updated equation.
2NaOH + CaBr2  Ca(OH)2 + 2NaBr
Are we now balanced?
Sure!
#R atom #P
2
2
1
2
Na
OH
Ca
Br
2
2
1
2
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Ok Try Balancing this equation:
C2H6 + O2  CO2 + H2O
Step 1. Total up the atoms
Step 2. Balance the #P Carbon
#R atom #P
2
6
2
C
H
O
2
2
5
#R atom #P
2
6
2
C
H
O
1
2
3
& Re-write the equation
C2H6 + O2  2CO2 + H2O
Are we done?
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Step 3. Carbons are balanced now but Hydrogen isn’t.
So, balance Hydrogen atoms next
Multiply #P Hydrogen by 3
Step 4. Re-write the eqn. &
Retotal the number of atoms
#R atom #P
2
6
2
C
H
O
2
6
7
#R atom #P
2
6
2
C
H
O
2
2 x3
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C2H6 + O2  2CO2 + 3H2O
Carbon and Hydrogen are now
balanced but oxygen isn’t.
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Step 5. To balance Oxygen multiply O by 3½
#R atom #P
Step 6. Re-write the eqn. &
2
Retotal the number
6
of atoms
3 ½ x2
C
H
O
2
6
7
C2H6 + 3½ O2  2CO2 + 3H2O
It looks like we’re balanced. But, are we?
No! We can’t have 3 ½ Oxygen molecules! Only whole
Numbers are allowed.
So what do we need to do to fix this?
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Step 7. Let’s clean this up by Multiply everything by 2
C2H6 + 3½ O2  2CO2 + 3H2O
x2
2C2H6 + 7 O2  4CO2 + 6H2O
#R atom #P
Step 8. Retotal #R and the
#P atoms
Are we balanced?
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12
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C
H
O
4
12
14
YES!
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Try this problem
NH4OH + FeCl3  Fe(OH)3 + NH4Cl
Start here. Recognize we
Have polyatomics but they
Appear on both sides of the
Equation.
#R atom #P
1
1
1
3
NH4
OH
Fe
Cl
1
3
1
1
OK … Now finish it up
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Answer to previous problem
3NH4OH + FeCl3  Fe(OH)3 + 3NH4Cl
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Types of Reactions
1.
2.
3.
4.
5.
Synthesis reactions
Decomposition reactions
Single displacement reactions
Double displacement reactions
Combustion reactions
You need to be able to identify each type.
1. Synthesis
Example C + O2
C + O O
General:

O C O
A + B  AB
Ex. Synthesis Reaction
Practice

Predict the products.
2 Na(s) + Cl2(g)  2 NaCl(s)
Mg(s) + F2(g) 
2 Al(s) +3 F2(g) 
MgF2(s)
2 AlF3(s)
• Now, balance them.
2. Decomposition
Example: NaCl
Cl Na

General:
Cl
+
Na
AB  A + B
Ex. Decomposition Reaction
3. Single Displacement
Example: Zn + CuCl2
Zn was oxidized
Cu
Cl
+
Cl
Zn
Went from neutral
(0) Zn
to (+2)

Cl
+
Cu
Cl
Cu was reduced
General:
Went from (+2) to
Neutral (0)
AB + C  AC + B
Ex. Single Replacement Reaction
Single Replacement Reactions


Write and balance the following single
replacement reaction equation:
Zn(s) +2 HCl(aq)  ZnCl2 + H2(g)
• 2 NaCl(s) + F2(g) 2 NaF(s) + Cl2(g)
•2 Al(s)+ 3 Cu(NO3)2(aq) 3 Cu(s)+ 2 Al(NO3)3(aq)
4. Double displacement
Example: MgO + CaS
Mg
+
O
General:
Ca
S

Mg
S
+
Ca
O
AB + CD  AD + CB
Double Replacement Reactions



Think about it like “foil”ing in algebra, first and
last ions go together + inside ions go together
Example:
AgNO3(aq) + NaCl(s)  AgCl(s) + NaNO3(aq)
Another example:
K2SO4(aq) + Ba(NO3)2(aq)  2 KNO3(aq) + BaSO4(s)
Practice

Predict the products.
5.
HCl(aq) + AgNO3(aq) 
CaCl2(aq) + Na3PO4(aq) 
Pb(NO3)2(aq) + BaCl2(aq) 
FeCl3(aq) + NaOH(aq) 
H2SO4(aq) + NaOH(aq) 
6.
KOH(aq) + CuSO4(aq) 
1.
2.
3.
4.
5. Combustion Reactions




Combustion reactions a hydrocarbon reacts with
oxygen gas.
This is also called
burning!!!
In order to burn
something you need the 3
things in the “fire
triangle”:
1) Fuel (hydrocarbon)
2) Oxygen
3) Something to ignite the
reaction (spark)
Combustion Reactions



In general:
CxHy + O2  CO2 + H2O
Products are ALWAYS
carbon dioxide and water.
(although incomplete burning
does cause some by-products
like carbon monoxide)
Combustion is used to heat
homes and run automobiles
(octane, as in gasoline, is C8H18)
Combustion

Example
•

C5H12 +8 O2 5 CO2 +6 H2O
Write the products and balance the
following combustion reaction:
•
C10H22 + O2 
Mixed Practice

1.
2.
3.
4.
5.
State the type & predict the products.
BaCl2 + H2SO4 
C6H12 + O2 
Zn + CuSO4 
Cs + Br2 
FeCO3 