Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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What is the SI unit of force?
a. | torr | c. | pound | b. | pascal | d. | newton |
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2.
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What does the constant bombardment of gas molecules against the inside walls of
a container produce?
a. | temperature | c. | pressure | b. | density | d. | diffusion |
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3.
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Why does a can collapse when a vacuum pump removes air from the can?
a. | The inside and outside forces balance out and crush the can. | b. | The unbalanced
outside force from atmospheric pressure crushes the can. | c. | The atmosphere
exerts pressure on the inside of the can and crushes it. | d. | The vacuum pump
creates a force that crushes the can. |
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4.
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Which instrument measures the pressure of an enclosed gas?
a. | barometer | c. | vacuum pump | b. | manometer | d. | torrometer |
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5.
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A pressure of 745 mm Hg equals
a. | 745 torr. | c. | 1 pascal. | b. | 1 torr. | d. | 745 pascal. |
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6.
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Standard temperature is exactly
a. | 100°C. | c. | 0°C. | b. | 273°C. | d. | 0 K. |
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7.
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Standard pressure is the pressure exerted by a column of mercury exactly
a. | 273 mm high. | c. | 760 cm high. | b. | 760 mm high. | d. | 1.00 m high. |
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8.
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Standard pressure is exactly
a. | 1 atm. | c. | 101.325 atm. | b. | 760 atm. | d. | 101 atm. |
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9.
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Three samples of gas each exert 740. mm Hg in separate 2 L containers. What
pressure do they exert if they are all placed in a single 2 L container?
a. | 247 mm Hg | c. | 1.48  103 mm Hg | b. | 740 mm
Hg | d. | 2.22  103 mm Hg |
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Use the table below to answer the following questions.
Water Vapor Pressure | Temperature (°C) | 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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10.
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A sample of gas is collected by water displacement at 600.0 mm Hg and 30°C. What is the partial pressure of the gas?
a. | 568.2 mm Hg | c. | 630 mm Hg | b. | 600.0 mm Hg | d. | 631.8 mm Hg |
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11.
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To observe the effects of changing pressure on the volume of a gas, factors that
must be kept constant are the gas's temperature and
a. | density. | c. | elasticity. | b. | quantity. | d. | kinetic energy. |
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12.
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The volume of a gas is 400.0 mL when the pressure is 1.00 atm. At the same
temperature, what is the pressure at which the volume of the gas is 2.0 L?
a. | 0.5 atm | c. | 0.20 atm | b. | 5.0 atm | d. | 800 atm |
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13.
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A sample of oxygen occupies 560. mL when the pressure is 800.00 mm Hg. At
constant temperature, what volume does the gas occupy when the pressure decreases to 700.0 mm
Hg?
a. | 80.0 mL | c. | 600. mL | b. | 490. mL | d. | 640. mL |
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14.
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V is the original volume, V' is the new volume, T is
the original Kelvin temperature, and T' is the new Kelvin temperature, how is
Charles's law expressed mathematically?
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15.
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The volume of a gas is 5.0 L when the temperature is 5.0°C. If the temperature is increased to 10.0°C without changing the pressure, what is the new volume?
a. | 2.5 L | c. | 5.1 L | b. | 4.8 L | d. | 10.0 L |
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16.
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The volume of a gas is 93 mL when the temperature is 91°C. If the temperature is reduced to 0°C
without changing the pressure, what is the new volume of the gas?
a. | 70. mL | c. | 120 mL | b. | 93 mL | d. | 273 mL |
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17.
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Why could the pressure of a sample of gas at a constant volume fall 75 mm
Hg?
a. | The container exploded. | c. | The temperature
decreased. | b. | The temperature increased. | d. | The volume increased. |
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18.
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If the temperature of a fixed quantity and volume of gas changes, what also
changes?
a. | pressure | c. | mass | b. | density | d. | formula |
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19.
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On a cold winter morning when the temperature is –13°C, 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 15°C?
a. | –1.5 atm | c. | 3.0 atm | b. | 1.7 atm | d. | 19.5 atm |
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20.
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The pressure of a sample of gas at 10.0°C
increases from 700. mm Hg to 900. mm Hg. What is the new temperature?
a. | 0°C | c. | 39.0°C | b. | 364°C | d. | 90.9°C |
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21.
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The volume of a sample of oxygen is 300.0 mL when the pressure is 1.00 atm and
the temperature is 27.0°C. At what temperature is the volume 1.00 L
and the pressure 0.500 atm?
a. | 22.0°C | c. | 0.50 K | b. | 45.0°C | d. | 227°C |
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22.
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Gay-Lussac recognized that at constant temperature and pressure, the volumes of
gaseous reactants and products
a. | always equal 1 L. | b. | add up to 22.4 L. | c. | equal
R. | d. | can be expressed as ratios of small whole numbers. |
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23.
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The law of combining volumes applies only to gas volumes
a. | measured at constant temperature and pressure. | b. | that equal 1
L. | c. | that equal 22.4 L. | d. | measured at
STP. |
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24.
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If 0.5 L of O2(g) reacts with H2 to produce 1 L of
H2O(g), what is the volume of H2O(g) obtained from 1 L of
O2(g)?
a. | 0.5 L | c. | 2 L | b. | 1.5 L | d. | 2.5 L |
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25.
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For reactants or products that are gases, the coefficients in the chemical
equation indicate
a. | the number of grams of each substance. | c. | molar volume. | b. | volume. | d. | density. |
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26.
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Volumes of gaseous reactants and products in a chemical reaction can be
expressed as ratios of small whole numbers
a. | if all reactants and products are gases. | b. | if standard
temperature and pressure are maintained. | c. | if constant temperature and pressure are
maintained. | d. | if each mass equals 1 mol. |
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27.
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The equation for the production of methane is C + 2H 2( g)  CH 4( g). How many
liters of hydrogen are needed to produce 20. L of methane? a. | 2.0 L | c. | 22.4 L | b. | 20. L | d. | 40. L |
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28.
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The principle that under similar pressures and temperatures, equal volumes of
gases contain the same number of molecules is attributed to
a. | Boyle. | c. | Avogadro. | b. | Graham. | d. | Dalton. |
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29.
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If the temperature of a container of gas remains constant, how could the
pressure of the gas increase?
a. | The mass of the gas molecules increase. | b. | The diffusion of the
gas molecules increases. | c. | The size of the container
increases. | d. | The number of gas molecules in the container
increases. |
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30.
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At constant temperature and pressure, gas volume is directly proportional to
the
a. | molar mass of the gas. | c. | density of the gas at STP. | b. | number of moles of
gas. | d. | rate of
diffusion. |
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31.
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The expression V = kn is a statement of
a. | Boyle's law. | c. | Graham's law of effusion. | b. | the law of combining
volumes. | d. | Avogadro's
law. |
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32.
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Avogadro's law led to the realization that the molecules of some
substances
a. | cannot react. | c. | are monatomic. | b. | are not composed of atoms. | d. | are diatomic. |
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33.
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In the expression V = kn, n represents
a. | the ideal gas constant. | c. | the number of moles of
gas. | b. | Avogadro's number. | d. | a constant. |
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34.
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According to Avogadro's law, 1 L of H2(g) and 1 L of
O2(g) at the same temperature and pressure
a. | have the same mass. | b. | have unequal volumes. | c. | contain 1 mol of gas
each. | d. | contain equal numbers of molecules. |
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35.
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The gas pressure inside a container decreases when
a. | the number of gas molecules is increased. | b. | the number of gas
molecules is decreased. | c. | the temperature is
increased. | d. | the number of molecules is increased and the temperature is
increased. |
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36.
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The standard molar volume of a gas is all of the following except
a. | the volume occupied by 1 mol of a gas at STP. | b. | equal for all gases
under the same conditions. | c. | 22.4 L at STP. | d. | dependent upon the
size of the molecules. |
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37.
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The standard molar volume of a gas at STP is
a. | 22.4 L. | c. | g-mol wt/22.4 L. | b. | g/22.4 L. | d. | 1 L. |
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38.
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At STP, the standard molar volume of a gas of known volume can be used to
calculate the
a. | number of moles of gas. | c. | gram-molecular
weight. | b. | rate of diffusion. | d. | gram-molecular volume. |
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39.
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Knowing the mass and volume of a gas at STP allows one to calculate the
a. | identity of the gas. | c. | condensation point of the gas. | b. | molar mass of the
gas. | d. | rate of diffusion of
the gas. |
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40.
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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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41.
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A 1.00 L sample of a gas has a mass of 1.25 g at STP. What is the mass of 1.00
mol of this gas?
a. | 0.855 g | c. | 22.4 g | b. | 1.25 g | d. | 28.0 g |
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42.
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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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43.
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The ideal gas law combines Boyle's law, Charles's law,
Gay-Lussac's Law and
a. | Graham's law. | c. | Raoult's law. | b. | Avogadro's law. | d. | Dalton's
principle. |
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44.
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All of the following equations are statements of the ideal gas law
except
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45.
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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. | –7°C | c. | 15°C | b. | 11°C | d. | 288°C |
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46.
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What is the pressure exerted by 1.2 mol of a gas with a temperature of 20.°C and a volume of 9.5 L?
a. | 0.030 atm | c. | 3.0 atm | b. | 1.0 atm | d. | 30. atm |
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47.
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A sample of gas at 25°C has a volume of 11 L and
exerts a pressure of 660 mm Hg. How many moles of gas are in the sample?
a. | 0.39 mol | c. | 9.3 mol | b. | 3.9 mol | d. | 87 mol |
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48.
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If a gas with an odor is released in a room, it can quickly be detected across
the room because it
a. | diffuses. | c. | is compressed. | b. | is dense. | d. | condenses. |
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Use the table below to answer the following questions.
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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49.
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How many times greater is the rate of effusion of molecular fluorine than that
of molecular bromine at the same temperature and pressure?
a. | 2.051 | c. | 4.450 | b. | 3.062 | d. | 7.280 |
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50.
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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. | 83.5 g/mol |
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