Transcript Dimensional Analysis

Dimensional Analysis
If you are traveling at 65 mi/h how long will it
take to travel 112 km?
If your car gets 28 miles per gallon how
many liters of gas will it take to travel the
112 km?
Density
What is the mass of a piece of gold with a
Volume of 1.0 L? The density of gold is
19.32 g/cm3
Kinetic Molecular Theory for an
Ideal Gas
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The particles are so small compared to the distances
between them that the volume of the particles can be
assumed to be negligible. (i.e. Particles have no
volume)
Particles are in constant random motion. The
collisions of the particles with the walls of the
containers are the cause of the pressure exerted by
the gas.
Particles are assumed to exert no forces on each
other. They neither attract nor repel each other.
The average kinetic energy of a collection of gas
particles is assumed to be directly proportional to the
Kelvin temperature of the gas. (KEavg = (3/2)RT
What is the effect on the volume of one mole
of an ideal gas if the pressure is doubled
and the Kelvin temperature is halved?
Dalton’s Law of Partial Pressures
A sample of KClO3(s) is decomposed by heating it
in a test tube. The oxygen gas produced is
collected over water at 22 °C and a total pressure
of 754 torr. The volume of the gas collected is
0.650 L and the vapor pressure of water at 22 °C
is 21 torr. Calculate the number of moles of
oxygen collected.
Also see ch. 5 # 67, 68, 103
0.30 g of a gas occupied a volume of
82.0 mL at 3.00 atm and 27 °C. Calculate
the molar mass of the gas.
Calculate the density of SF6 at 1.0 atm and
0.0 °C.
At 0 °C and 1.0 atm, 1.0 L of Br2 reacts
completely (i.e. exactly) with 3.0 L of F2
producing 2.0 L of a product. What is the
formula of the product?
Lung capacity for a typical person is 2.0 L. If
air at 20.0 °C and 1.0 atm fills the lungs,
how many molecules of air are present?
An atomic bomb needs 4.0 moles of
Uranium. How many grams of U are
needed? Atoms?
Determine mass % Al and O in aluminum
oxide.
A certain gas contains 81.10% boron and
18.90 % hydrogen by mass. The molar
mass of the gas is 53.4 g/mol. Determine
the empirical formula and molecular formula
of the gas.
Glucose contains only C, H and O. When
1.00 g of glucose is combusted it yields
1.47 g of CO2 and 0.600 g of H2O. Glucose
has a molar mass of 180.16 g/mol. What is
The molecular formula of glucose? What is
the mass % of C, H, and O?
Stoichiometry – using a balanced chemical
Equation to determine how much reactant or
product is consumed or produced in a
chemical reaction.
C12H22O11 + H2O2  H2O + CO2
How many grams of CO2 are produced from
The combustion, in air, of 10.00 mL of
benzene (C6H6)? The density of benzene is
0.879 g/mL
3A+BC+2D
If 4.0 mol of A are reacted with 2.0 mol of B
What is the limiting reactant? How many
Moles of C and D can be produced?
Fe2O3(s) + CO(g)  Fe(s) + CO2(g)
If 2.0 kg of Fe2O3 and 1.5 kg of CO are
reacted what is the maximum amount of iron
that could be produced?
If the actual yield of iron is 650 g what is the
percent yield?
Solubility Rules
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Most nitrate salts are soluble.
Most salts of alkali metals and ammonium cations are soluble.
Most chloride, bromide, and iodide salts are soluble.
Exceptions: salts containing Ag+, Pb2+, and Hg22+ ions are
insoluble.
Most sulfate salts are soluble.
Exceptions: salts containing Ca2+, Ba2+, Pb2+, and Hg22+ ions are
insoluble.
Most hydroxide salts are insoluble.
Exceptions: hydroxides containing alkali metals, Ba2+, Sr2+ and
Ca2+ ions are soluble.
Most sulfide, carbonate, chromate, and phosphate salts are
insoluble.
Exceptions: salts of alkali metals and ammonium cations are
soluble.
How many moles of ions are present in a
2.0 L solution of 1.0 M Ca(OH)2?
How much H2O is needed to dilute 5.0 L of
a 2.0 M solution of NaCl to 0.50 M?
A 0.6025 g sample of a compound
containing chloride ion was dissolved in H2O
and the chloride precipitated by adding
excess silver nitrate. The precipitant of
silver chloride was found to weigh 0.7134 g.
Calculate the mass % of chloride in the
sample.
What volume of 0.050 M sodium phosphate
Solution is needed to react completely with
30.0 mL of 0.10 M silver nitrate?
What mass of precipitant would form from
30.0 mL of 0.10 M AgNO3 using excess
Na3PO4 solution?
What volume of 0.200 M HCl is needed to
titrate 20.0 mL of 0.350 M NaOH?
When titrating 0.150 M HCl with a calcium
hydroxide solution of an unknown
concentration, 25.0 mL of the base are
required to neutralize 35.0 mL of the acid.
Calculate the molarity of the base.
A chemist dissolves 0.300 g of an unknown
monoprotic acid in a convenient volume of
water. She finds that 14.60 mL of 0.426 M
sodium hydroxide are required to neutralize
the acid. What is the molar mass of the
acid?