Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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Unlike in an ideal gas, in a real gas a. | all particles
move in the same direction. | b. | all particles have the same kinetic
energy. | c. | the particles cannot diffuse. | d. | the particles
exert attractive forces on each other. | | |
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2.
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Which
is NOT an assumption of the kinetic-molecular theory? a. | Matter is
composed of tiny particles. | b. | The particles of matter are in continual
motion. | c. | The total kinetic energy of colliding particles remains
constant. | d. | When individual particles collide, energy is
transferred. | | |
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3.
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Diffusion between two gases occurs most rapidly if the gases are at a a. | high temperature
and the molecules are small. | b. | low temperature and the molecules are
large. | c. | low temperature and the molecules are
small. | d. | high temperature and the molecules are
large. | | |
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4.
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Why
doesn't a gas at a low temperature behave like an ideal gas? a. | There is too
much space between the particles. | b. | The attractive forces are too weak. | c. | The kinetic
energy of the particles is too low. | d. | The particles undergo chemical
reactions. | | |
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5.
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Two
gases have the same temperature but different pressures. The kinetic-molecular theory does NOT
predict that a. | molecules in
both gases have the same average kinetic energies. | b. | molecules in the
low-pressure gas travel farther before they collide with other molecules. | c. | both gases have
the same densities. | d. | all collisions of the molecules are
elastic. | | |
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6.
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The
volume of a gas is 400. mL at 30.0ºC. If the temperature is increased to 50.0ºC without
changing the pressure, what is the new volume of the gas? a. | 375
mL | c. | 426
mL | b. | 400
mL | d. | 600
mL | | | | |
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7.
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On a
cold winter morning when the temperature is –13ºC, the air pressure in an automobile tire
is 1.5 atm. If the volume does not change, what is the pressure after the tire has warmed to
15ºC? a. | –1.5
atm | c. | 3.0
atm | b. | 1.7
atm | d. | 19.5
atm | | | | |
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Water Vapor Pressure
Temperature (ºC) | Pressure (mm
Hg) | 0 | 4.6 | 5 | 6.5 | 10 | 9.2 | 15 | 12.8 | 20 | 17.5 | 25 | 23.8 | 30 | 31.8 | 35 | 42.2 | 40 | 55.3 | 50 | 92.5 | | |
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8.
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What
is the partial pressure of water vapor in oxygen gas collected by water displacement at 10ºC and
750 mm Hg? a. | 9.2 mm
Hg | c. | 750 mm
Hg | b. | 740.8 mm
Hg | d. | 759.2 mm
Hg | | | | |
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9.
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In
the equation H2(g) + Cl2(g) ® 2HCl(g),
one volume of hydrogen yields how many volumes of hydrogen chloride?
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10.
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A
1.00 L sample of a gas has a mass of 1.92 g at STP. What is the molar mass of the
gas? a. | 1.92
g/mol | c. | 22.4
g/mol | b. | 19.2 g/mol | d. | 43.0 g/mol | | | | |
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11.
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The
ideal gas law is equivalent to Charles's law when a. | the number of moles and the pressure are
constant. | b. | the number of moles and the temperature are
constant. | c. | the volume equals 22.4 L. | d. | R equals
zero. | | |
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12.
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The
ideal gas law is equivalent to Boyle's law when a. | Avogadro's number is reached. | b. | R equals
zero. | c. | the pressure is 1 atm. | d. | the number of
moles and the temperature are constant. | | |
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13.
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Calculate the approximate temperature of a 0.50 mol sample of gas at 750 mm Hg and a
volume of 12 L. a. | –7ºC | c. | 15ºC | b. | 11ºC | d. | 288ºC | | | | |
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14.
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A gas
sample with a mass of 2.50 g is collected at 20.0ºC and 732.5 mm Hg. The volume is 1.28 L. What
is the molar mass of the gas? a. | 1.26 g/mol | c. | 13.7 g/mol | b. | 2.04
g/mol | d. | 48.8
g/mol | | | | |
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15.
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The
equation for the complete combustion of methane is CH4(g) +
2O2(g) ® 2H2O(g) + CO2(g). If 50 L of
methane at STP are burned, what volume of carbon dioxide will be produced at STP? a. | 16.6
L | c. | 50
L | b. | 25
L | d. | 100
L | | | | |
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Element | Atomic mass | Argon | 39.948 | Bromine | 79.904 | Carbon | 12.011 | Chlorine | 35.453 | Fluorine |
18.998 | Helium | 4.0026 | Hydrogen | 1.0079 | Nitrogen |
14.007 | Oxygen | 15.999 | | |
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16.
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A
sample of helium diffuses 4.57 times faster than an unknown gas diffuses. What is the molar mass of
the unknown gas? a. | 12
g/mol | c. | 38.8
g/mol | b. | 18.2 g/mol | d. | 83.6 g/mol | | | | |
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17.
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Each stopped flask below contains 2 liters of a gas at STP.
Each gas has the same:
a. | density
| c. | number of molecules
| b. | mass
| d. | number of
atoms
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Problem
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18.
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Given
the equation:
Zn (s) + 2 HCl
(aq) --> ZnCl2 (aq) + H2(g)
If 520 mL of H2 is collected over water at 28oC and the
atmospheric pressure is 1.0 atm, how many g of Zn was used at the start of the reaction? (vapor
pressure of water at 28oC is 28.3 mmHg).
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19.
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Calculate the volume of 10.8 g of CO2 at STP.
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20.
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A 2.1
L flask contains 4.65 g of gas at 1 atm and 27oC, what is the density and molar mass of
the gas?
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