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Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. When a sealed 2 L flask is heated, what happens to the gas molecules?
a. They move closer together.
b. Their kinetic energy decreases.
c. They collide more often with the sides of the flask.
d. They decrease their molecular motion.
e. Their intermolecular forces increase.
____
2. Which of the following are characteristics of gases?
I. They have a variable shape.
II. They are compressible.
III. They have a constant volume.
IV. They have a high viscosity.
a. I and II
b. I, II, and III
____
c. I and IV
d. II and III
e. I, II, III, and IV
3. Which of the following are characteristics of atoms and molecules in the gaseous state?
I. They expand as the temperature is increased,
II. They are compressible,
III. They have high densities,
IV. They are miscible,
a. I and II
b. I, II, and III
c. I and IV
d. I and III
e. I, II, and IV
____
4. Which of the following statements best explains why gases can easily expand?
a. Molecules of a gas have small amounts of space between them.
b. Molecules of a gas have little volume.
c. Molecules of a gas are in constant motion.
d. Molecules of a gas exhibit random rotational motion.
e. Molecules of a gas are considered point masses.
____
5. Which is not a correct statement of the kinetic molecular theory as it relates to gases?
a. Gas particles are in constant motion.
b. Gas particles travel in straight-line motion.
c. Gas particles exhibit elastic collisions.
d. Gas particles exert strong attractive and repulsive forces.
e. Gas particles are considered point masses.
____
6. Which property or properties of gases accounts for the observation that gases are miscible?
I. Gas particles have no volume.
II. Gas particles exhibit elastic collisions.
III. Gas particles are in constant random motion.
IV. Gas particles do not exert attractive or repulsive forces on one another.
a. I only
b. I and II
c. I, II, and III
d. III and IV
e. I and IV
____
7. Based on an understanding of intermolecular forces, which molecule would most likely be a gas at room
temperature?
a. C3H8
b. C4H10
c. C5H12
d. C6H14
e. C8H18
____
8. Which type of intermolecular force is considered to be the weakest force that influences the state of matter?
a. ionic bonding
d. hydrogen bonding
b. covalent bonding
e. temporary dipole forces
c. dipole-dipole force
____
9. A gas sample is confined in a 1 L container. Which of the following will occur if the temperature is
increased?
I. The kinetic energy will increase.
II. The pressure will decrease.
III. The density of the gas will decrease.
IV. The molecular motion will increase.
a. I only
b. II only
c. II and III
d. III and IV
e. I and IV
____ 10. A gas sample is confined in a 4 L balloon. Which of the following will occur if the pressure on the balloon is
increased at a constant temperature?
I. The volume of the balloon will increase.
II. The kinetic energy of the molecules of the gas in the balloon will decrease.
III. The density of the gas will increase.
a. I only
b. II and III
c. I and II
d. III only
e. I, II, and III
____ 11. Which statement is not true?
a. The average kinetic energies of molecules from samples of different “ideal” gases is the
same at the same temperature.
b. The molecules of an ideal gas are relatively far apart.
c. All molecules of an ideal gas have the same kinetic energy at constant temperature.
d. Molecules of a gas undergo many collisions with each other and the container walls.
e. Molecules of greater mass have a lower average speed than those of less mass at the same
temperature.
____ 12. Which of the following gases would have the highest density at the same temperature, pressure, and volume?
a. H2
b. CClF3
c. CO2
d. C2H6
e. CF4
____ 13. A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original
pressure was 100 kPa, what is the new pressure?
a. 10 kPa
c. 100 kPa
e. 100 kPa
b. 50 kPa
d. 200 kPa
____ 14. A sample of gas is in a sealed flexible container at a fixed temperature. If the pressure on the container is
increased by three, then the volume will
a. increase by a factor of 3
b. increase by a factor of 6
c. decrease by a factor of 1
d. decrease by a factor of 3
e. decrease by a factor of 6
____ 15. Which of the following represents the lowest pressure?
a. 1.5 atm
c. 200 kPa
b. 650 mmHg
d. 42 PSI
e. 900 torr
____ 16. A given mass of oxygen at room temperature occupies a volume of 500.0 mL at 1.50 atm pressure. What
pressure must be applied to compress the gas to a volume of only 150.0 mL?
a. 500 atm
c. 5.00 atm
e. 0.500 atm
b. 150 atm
d. 1.50 atm
____ 17. A sample of the inert gas krypton has its pressure tripled while its temperature remains constant. If the
original volume is 12 L, what is the final volume?
a. 4 L
b. 6 L
c. 9 L
d. 36 L
e. 48 L
____ 18. Which of the following changes would increase the pressure of a gas in a sealed container?
I. adding more moles of gas to the container
II. The container size is decreased.
III. The temperature is increased.
IV. The external pressure is decreased.
a. I only
b. I and II
c. I, II, and III
d. II and IV
e. II, III, and IV
____ 19. Which statement best describes the behaviour of the volume of a fixed mass of gas in a sealed syringe?
a. It decreases as the temperature of the syringe increases.
b. It decreases as the syringe is pulled outward.
c. It increases when the temperature of the syringe is increased.
d. It increases when the syringe is pushed inward.
e. It does not change when the temperature or pressure in the syringe changes.
____ 20. Decreasing the pressure of an ideal gas at constant mass and temperature will cause which of the following to
increase?
I. the molar mass of the gas
II. the volume of the gas
III. the density of the gas
IV. the average kinetic energy of the gas
a. I and II
b. II only
c. II and III
d. I and IV
e. I, II, and IV
____ 21. Decreasing the temperature of an ideal gas at constant mass will cause which of the following to decrease
I. molar mass
II. the volume of the gas
III. the density of the gas
IV. the average kinetic energy of the gas
V. the pressure of the gas
a. II, III, and IV
b. III, IV, and V
c. I, II, and III
d. II, IV, and V
____ 22. What Kelvin temperature is equal to 55C?
a. –218 K
b. 5 K
c. 218 K
e. II, III, IV, and V
d. 328 K
e. –55 K
____ 23. According to Boyle’s law, a gas will have a decreased ____________ if the pressure is increased.
a. volume
b. temperature
c. average kinetic energy
d. pressure
e. mass
____ 24. According to Gay-Lussac’s law, a gas will have a decreased __________ if the temperature is decreased.
a. volume
b. temperature
c. average kinetic energy
d. pressure
e. mass
____ 25. According to Charles’s law, a gas will have a decreased ___________ if the volume is reduced.
a. volume
d. pressure
b. temperature
e. mass
c. average kinetic energy
____ 26. The kinetic molecular theory states that there is a direct relationship between which two of the following?
I. decreased volume
II. decreased temperature
III. decreased average kinetic energy
IV. decreased pressure
V. decreased mass
a. I and IV
b. I and V
c. II and III
d. II and IV
e. I and III
____ 27. Which of the following pairs are not directly proportional to each other, assuming no other conditions are
varied?
I. decreased volume
II. decreased temperature
III. decreased average kinetic energy
IV. decreased pressure
V. decreased mass
a. I and II
b. II and IV
c. I and V
d. II and III
e. I and IV
____ 28. Which of the following statements concerning the molecular motion of gases is not true?
a. The kinetic energy of all gas particles is the same.
b. Gas molecules collide elastically.
c. Gas molecules exhibit rotational, vibrational, and translational motion.
d. Gas particles are in constant random motion.
e. Gas particles travel in straight lines.
____ 29. Which statement is not true with respect to liquids and gases?
a. Gases and liquids both display variable shape.
b. Gases are compressible, and liquids are almost incompressible.
c. Gases have much lower densities than liquids do.
d. Gases are miscible, and some liquids are immiscible with one another.
e. Gases expand as their temperature increases, but liquids do not.
____ 30. When 500 mL of a gas at constant pressure is heated from 25C to 75C, the volume must be multiplied by
a.
c.
e.
b.
d.
____ 31. When a sample of a gas at a pressure of 200 kPa and constant volume is heated from 30C to 80C, the
pressure must be multiplied by
a.
b.
c.
d.
e.
____ 32. Which of the following statements concerning atmospheric pressure is not true?
a. It decreases with altitude.
b. It can be measured with a barometer.
c. It affects the lifting ability of a suction pump.
d. It is higher on a mountain than at sea level.
e. It is unaffected by weather patterns.
____ 33. A 3 L sample of a noble gas is stored in a container with a constant pressure. If the temperature (in K) of the
gas is tripled, what is the new volume of the gas, assuming the container is flexible?
a. 3 L
b. 6 L
c. 9 L
d. 1.5 L
e. 1 L
____ 34. As temperature is increased, the pressure of a gas increases in a fixed volume. In terms of the kinetic
molecular theory, this is explained by the fact that
a. gas particles strike the container walls more frequently
b. gas particles have little attractive or repulsive forces between them
c. gas particles display an increase in vibrational energy
d. gas particles are considered point masses
e. gas particles have a lower density at higher temperatures
____ 35. In which of the following situations is it impossible to predict whether the pressure of a gas will increase,
decrease, or stay the same without doing mathematical calculations?
a. A gas sample is cooled.
b. A gas sample is cooled, and the volume of the gas decreases.
c. A gas sample is heated, and some of the gas is added.
d. A gas sample is heated, and the volume of the gas decreases.
e. Additional gas is added to the gas sample.
____ 36. In which of the following situations is it impossible to predict whether the volume of a gas will increase,
decrease, or stay the same without doing mathematical calculations?
a. The pressure of the gas is increased.
b. The temperature of the gas is decreased.
c. The pressure of the gas is increased and the temperature of the gas is decreased.
d. The pressure of the gas is increased and the temperature of the gas is increased.
e. More gas is added to the container.
____ 37. The pressure of an ideal gas is measured at several different temperatures in degrees Kelvin. When a graph of
the data is made, which of the following will be not true?
a. Pressure (dependent variable) will be plotted on the x-axis and temperature (independent
variable) will be plotted on the y-axis.
b. The graph will display a linear relationship.
c. P/T will be a constant.
d. As temperature increases, pressure increases.
e. If extrapolated, the graph will pass through the point (0, 0).
____ 38. According to Boyle’s law, which of the following will occur if the pressure on a gas is increased?
a. The volume of gas will increase.
b. The volume of gas will decrease.
c. The amount (in moles) of gas will increase.
d. The temperature of the gas will increase.
e. The temperature of the gas will decrease.
____ 39. According to the Gay-Lussac’s law, which of the following will occur if the temperature on a gas is
increased?
a. The volume of the gas will increase.
b. The volume of the gas will decrease.
c. The amount (in moles) of the gas will increase.
d. The pressure of the gas will increase.
e. The pressure of the gas will decrease.
____ 40. According to Charles’s law, which of the following will occur if the temperature of a gas is decreased?
a. The pressure of the gas will decrease.
b. The pressure of the gas will increase.
c. The mass of the gas will increase.
d. The volume of the gas will increase.
e. The volume of the gas will decrease.
____ 41. Which of the following statements conflicts with the kinetic molecular theory of gases?
a. There are no intermolecular forces between gas particles.
b. Gas particles occupy a negligible volume compared with the volume of their container.
c. The average kinetic energy of the gas particles is proportional to the temperature.
d. Gas particles lose energy only when they collide with the walls of the container.
e. Gas particles are in constant, random motion.
____ 42. The term absolute zero refers to which combination of the following?
I. the temperature at which water freezes
II. the temperature at which a gas has zero volume
III. the temperature at which a gas has zero pressure
IV. –273.15C
a. I only
b. II only
c. II and IV
d. II, III, and IV
e. I, III, and IV
____ 43. Which of the following will increase when the temperature of a fixed amount of gas at a constant volume is
increased?
I. pressure of the gas
II. kinetic energy of molecules
III. space between molecules
a. I only
b. II only
c. I and III
d. I and II
e. II and III
____ 44. A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remains constant. If
the initial volume is 400 mL, what is the final volume?
a. 20 mL
c. 200 mL
e. 800 mL
b. 133 mL
d. 400 mL
____ 45. Which of the following scientists is credited with discovering the mathematical relationship between the
pressure and volume of a gas?
a. Evangelista Torricelli
d. Jacques Charles
b. Galileo Galilei
e. Joseph Louis Gay-Lussac
c. Robert Boyle
____ 46. Which of the following scientists is credited with discovering the mathematical relationship between the
temperature and pressure of a fixed volume of a gas?
a. Evangelista Torricelli
d. Jacques Charles
b. Galileo Galilei
e. Joseph Louis Gay-Lussac
c. Robert Boyle
____ 47. If the temperature of a fixed mass of a gas is kept constant while the volume is decreased in a flask, then
a. the number of collisions with walls of the flask decreases
b. the number of collisions with the walls of the flask increases
c. the average kinetic energy of the particles increases
d. the average kinetic energy of the molecules decreases
e. the pressure of the gas will decrease
____ 48. Which of the following formulas best describes Boyle’s law?
a. P1T1 = P2T2
c. P1V1 = P2V2
b. V1T1 = V2T2
e.
d. P1V2 = P2V1
____ 49. Which of the following formulas best describes Charles’s’s law?
a.
c.
e. T1V1 = T2V2
b.
d. P1V1 = P2V2
____ 50. Which of the following formulas best describes Gay-Lussac’s law?
a.
c.
e. T1V1 = T2V2
b.
d. P1V1 = P2V2
____ 51. According to the kinetic molecular theory, gas molecules are in random motion. This helps to explain which
property of gases?
a. They are compressible.
b. They have a low density.
c. They occupy the volume of the container they are placed in.
d. They are miscible with each other.
e. They contract when the temperature is decreased.
____ 52. Which of the following statements is (are) correct?
I. The volume of a gas is inversely proportional to its pressure.
II. The pressure of a gas is inversely proportional to it absolute temperature.
III. The volume of a gas is directly proportional to its absolute temperature.
a. I only
b. II only
c. III only
d. I and II
e. I and III
____ 53. The density of a gas in a flexible container
a. varies inversely with pressure at constant temperature
b. varies directly with the absolute temperature at constant pressure
c. varies inversely with the absolute temperature at constant pressure
d. decreases as the mass of the gas increases
e. does not vary with temperature or pressure
____ 54. A pressure of 2.00 atm is the same as a pressure of
a. 101 kPa
c. 760 kPa
b. 202 kPa
d. 1520 kPa
e. 29.4 kPa
____ 55. A given mass of a gas in a rigid container is heated from 200C to 400C. Which of the following responses
best describes what will happen to the volume of the gas?
a. The volume will decrease by a factor of 2.
b. The volume will increase by a factor if of 2.
c. The volume will increase by a factor of about 4.
d. The volume will decrease by a factor of about two thirds.
e. The volume will increase by a factor of about one and a third.
____ 56. Ideal gases are assumed to have which of the following, according to the kinetic molecular theory?
a. no pressure
d. no motion
b. no volume
e. no space between molecules
c. no mass
____ 57. A balloon is filled with neon gas. If the balloon were cooled, which of the following would result?
I. decrease in volume
II. decrease in density
III. decrease in pressure
IV. decrease in mass
a. I and II
b. II only
c. I and III
d. I, II, and III
e. II and IV
____ 58. A balloon is filled with oxygen gas. If the balloon were placed under higher external pressure at constant
temperature, which of the following would result?
I. increase in volume
II. increase in density
III. increase in mass
a. I only
b. II only
c. III only
d. I and II
e. I, II, and III
____ 59. Which of the following gases would be expected to display the greatest intermolecular forces?
a. NH3
b. CH4
c. HCl
d. Ne
e. He
____ 60. Which of the following scientists is credited with receiving a patent for a suction pump?
a. Evangelista Torricelli
d. Jacques Charles
b. Galileo Galilei
e. Joseph Louis Gay-Lussac
c. Robert Boyle
____ 61. Which of the following scientists is credited with creating a new temperature scale based on absolute zero, the
lowest temperature possible of –273.15C?
a. Joseph Louis Gay-Lussac
d. Jacques Charles
b. Galileo Galilei
e. Lord Kelvin William Thomson
c. Robert Boyle
____ 62. A rigid metal tank contains neon gas. Which of the following applies to the gas in the tank when some neon is
removed at constant temperature?
a. The volume of the gas decreases.
b. The pressure of the gas decreases.
c. The average speed of the gas molecules decrease.
d. The total number of gas molecules remains the same.
e. The average distance between the gas molecules decreases.
____ 63. Doubling the absolute temperature of a fixed mass of a gas in a rigid container will cause
I. the pressure of the gas to double
II. the density of the gas to double
III. the volume of the gas to double
a. I only
b. II only
c. I and II
d. II and II
e. I, II, and III
____ 64. To expand a 2 L sample of gas to 4 L, it is necessary to
a. double the temperature in degrees Celsius
b. double the pressure
c. halve the pressure
d. halve the temperature in degrees Celsius
e. halve the amount (in moles) of the gas
____ 65. Which of the following is standard atmospheric pressure?
a. 100 kPa
c. 2 atm
b. 1.00 bar
d. 10 psi
e. 760 mmHg
____ 66. The mass of a fixed quantity of gas
a. increases when the volume increases at constant temperature
b. decreases when the absolute temperature decreases at constant pressure
c. increases when the volume is decreased and the temperature is decreased
d. increases when the pressure is raised and the temperature is constant
e. does not change at any temperature and pressure
____ 67. In a sealed 2 L container of gas, the temperature is lowered. This causes the particles of gas to
a. increase their translational motion
b. move further apart
c. collide more frequently with the walls of the container
d. decrease their kinetic energy
e. increase their vibrational and rotational motion
____ 68. A property of all gases is that
a. they are odourless
b. they are clear and colourless
c. they are incompressible
d. they have low viscosities
e. they are immiscible
____ 69. Which of the following is the property of the element mercury that makes it useful in barometers?
a. It is a metal and conducts electricity.
b. It is a liquid at room temperature and has a high density.
c. It is a metal and is magnetic.
d. It is a nonmetal and dissolves in water.
e. It is a metal and adheres to glass well.
____ 70. According to the kinetic molecular theory, gas particles have ___________attractive forces and have and
exhibit ____________ collisions.
a. negligible, elastic
d. negligible, inelastic
b. large, elastic
e. small, elastic
c. small, inelastic
____ 71. Which of the following conditions will cause a decrease in the pressure of a gas?
I. decreasing the temperature
II. decreasing the volume
III. removing some amount of the gas
a. I only
b. II only
c. III only
d. I and II
____ 72. What volume will be occupied by 40.2 g of neon gas at STP?
a. 11.2 L
c. 33.6 L
b. 22.4 L
d. 44.8 L
e. I and III
e. 56.0 L
____ 73. Under what conditions will neon deviate from the ideal gas?
a. high temperature and high pressure
b. high temperature and low pressure
c. low temperature and high pressure
d. low temperature and low pressure
e. at moderate temperature and pressure
____ 74. Hydrogen gas was collected over water at a temperature of 25C, and the pressure of the room was 786
mmHg. If the vapour pressure of water at 25C is 25 mmHg, what is the partial pressure of hydrogen gas at
this temperature?
a. 25 mmHg
c. 811 mmHg
e. 836 mmHg
b. 786 mmHg
d. 761 mmHg
____ 75. Which of the following conditions would be most likely to cause the ideal gas law to fail?
I. low pressure
II. low temperature
III. large volume
a. I only
b. II only
c. III only
d. I and II
e. II and III
____ 76. Which of the following gas laws states, “equal volumes of gases at the same temperature and pressure contain
the same number of molecules”?
a. ideal gas law
d. law of combining volumes
b. combined gas law
e. Avogadro’s law
c. Dalton’s law of partial pressures
____ 77. The ideal gas law can be used to derive all of the following except
a. Boyle’s law
d. Avogadro’s law
b. Charles’s law
e. Dalton’s law of partial pressures
c. Gay-Lussac’s law
____ 78. A gas has a density at STP of 3.21 g/L. The most reasonable formula for this gas is
a. Ne
b. O2
c. CO2
d. Cl2
e. HCl
____ 79. A gas has a density at STP of 1.98 g/L. The most reasonable formula for this gas is
a. He
b. CO2
c. N2
d. NH3
e. CH4
____ 80. "The total pressure in a mixture of unreacting gases is equal to the sum of the partial pressures of the
individual gases" is a statement of __________________.
a. Charles’s law
d. Avogadro’s law
b. Boyle’s law
e. Dalton’s law of partial pressures
c. the ideal gas law
____ 81. At moderate to high pressures, the measured pressure exerted by CO2 gas is less than that predicted by the
ideal gas equation. This is mainly because
a. such high pressures cannot be accurately measured
b. CO2 will condense to a liquid at 200 atm pressure
c. gas phase collisions prevent CO2 molecules from colliding with the walls of the container
d. of attractive intermolecular forces between CO2 molecules
e. the volume occupied by the CO2 molecules themselves becomes significant
____ 82. Which of the following gases has the greatest density at STP?
a. He
b. Ar
c. H2
d. F2
e. Cl2
____ 83. Which of the following gases has the lowest density at STP?
a. H2
b. Ne
c. Cl2
d. CH4
e. NH3
____ 84. Of the following gases, which will behave most like an ideal gas?
a. He
b. HCl
c. NH3
d. H2O
e. CO
____ 85. According to the ideal gas law, if the amount of a gas is doubled and the absolute temperature of the gas is
also doubled while the volume remains unchanged, then the pressure of a gas should
a. increase by two times
b. decrease by two times
c. increase by four times
d. increase by eight times
e. No change; the effects cancel each other out.
____ 86. If the combined gas law were rearranged to solve for T2, it would become
a.
c.
e.
b.
d.
____ 87. If the combined gas law were rearranged to solve for P1, it would become
a.
c.
e.
b.
d.
____ 88. Use the combined gas law. The pressure of a gas is raised from 1 atm to 3 atm and the temperature is raised
from 100 K to 200 K. The volume of the gas will
a. remain the same
d. decrease by half
b. increase by two times
e. increase by six times
c. increase by four times
____ 89. Use the combined gas law. The pressure of a gas is decreased from 400 kPa to 200 kPa and the temperature is
raised from 200 K to 300 K. The volume of the gas will
a. decrease by half
d. increase by three times
b. remain the same
e. increase by four times
c. increase by two times
____ 90. A 155 mL sample of gas was initially at a pressure of 101 kPa at 50C. If the pressure were increased to 250
kPa at 100C, then the new volume could be calculated by
a.
d.
b.
e.
c.
____ 91. A 250 mL sample of gas was initially at a pressure of 101 kPa at 80C. If the volume decreases to 100 mL at
50C, then the new pressure could be calculated by
a.
d.
b.
e.
c.
____ 92. Dinitrogen pentoxide decomposes according to the following equation:
N2O5(g) → 4NO2(g) + O2(g)
According to Avogadro’s law, if 6 L of dinitrogen pentoxide decomposed, then the volume of nitrogen
dioxide and oxygen gas produced would be
a. 4 L NO2 , 1 L O2
d. 8 L NO2 , 4 L O2
b. 6 L NO2 , 3 L O2
e. 8 L NO2 , 2 L O2
c. 12 L NO2 , 3 L O2
____ 93. During a chemical reaction, oxygen gas was produced at 25C and a pressure of 99 kPa. If the volume of
oxygen gas collected was 250 mL, the amount (in moles) of gas produced would be
a.
d.
b.
e.
c.
____ 94. A reaction produced 0.5 mol of sulfur dioxide gas. If the temperature of the gas was 80C at a pressure of 101
kPa, then the volume produced would be
a.
d.
b.
e.
c.
____ 95. Which of the following statements corresponds to Avogadro’s law?
a. The sum of the volume of gaseous reactants equals the sum of the volume of gaseous
products.
b. The product of pressure and volume is directly related to the amount of a gas at constant
temperature.
c. Volume is directly related to the amount of a gas at constant temperature and pressure.
d. Pressure is directly related to the amount of a gas at constant volume and temperature.
e. Temperature is directly related to the amount of a gas at constant volume and temperature.
____ 96. Consider the following gas laws:
I. Dalton’s law of partial pressures
II. Avogadro’s law
III. law of combining volumes
IV. ideal gas law
V. Gay-Lussac’s law
Which of these gas laws involve the amount (in moles) of a gas as part of the mathematical relationship?
a. I only
b. II only
c. I, II, and III
d. II and IV
e. V only
____ 97. It has been observed experimentally that when water is decomposed by electrolysis into hydrogen and oxygen
gas, two volumes of hydrogen are collected for every one volume of oxygen. This observation is best
explained by which of the following laws?
a. ideal gas law
d. Avogadro’s law
b. Gay-Lussac’s law
e. Charles’s law
c. Dalton’s law of partial pressures
____ 98. Hydrogen chloride gas is decomposed into its component gases hydrogen and chlorine gas at STP. Which of
the following statements concerning this reaction is true?
a. Two volumes of hydrogen gas will be produced for every volume of chlorine gas.
b. Two volumes of chlorine gas will be produced for every volume of hydrogen gas.
c. Two volumes of hydrogen chloride gas produce two volumes of hydrogen gas.
d. Two volumes of hydrogen chloride gas produced two volumes of chorine gas.
e. Equal volumes of hydrogen and chlorine gas are produced.
____ 99. Liquid water can undergo decomposition by electrolysis to produce hydrogen and oxygen gas. Which of the
following statements concerning this reaction is false?
a. Two volumes of hydrogen are produced for every volume of oxygen gas.
b. If 1 mol of water is decomposed, this will produce 12.2 L of hydrogen gas.
c. If 2 mol of water are decomposed, this will produce 22.4 L of oxygen gas.
d. If the volume of hydrogen gas produced was 22.4 L, then 1 mol of water was decomposed.
e. If the volume of oxygen gas produced was 22.4 L, then 2 mol of water was decomposed.
____ 100. Standard temperature air pressure is defined as
a. 273.15 K, 100 kPa
d. 298.15 K, 100 kPa
b. 0C, 100 kPa
e. 25C, 101.325 kPa
c. 273.15 K, 101.325 kPa
____ 101. Which of the following is not considered to be a criteria air contaminant?
a. carbon monoxide
d. volatile organic compounds (VOCs)
b. carbon dioxide
e. nitrogen oxides
c. sulfur dioxide
____ 102. Ground-level ozone is produced as a result of the production of which of the following criteria air
contaminants?
a. particulate materials
d. volatile organic compounds
b. nitrogen oxides
e. sulfur dioxide
c. carbon monoxide
____ 103. When collecting a gas over water using a graduated cylinder, which of the following is false?
a. Gas displaces the water in the graduated cylinder.
b. Gas rises to the top of the graduated cylinder because it is less dense than water.
c. Gaseous water vapour must be accounted for using Dalton’s law of partial pressures.
d. The collection of trapped air must be avoided.
e. The solubility of the gas in water has no effect on the volume of gas collected.
____ 104. If equal masses of O2(g) and N2(g) are in separate containers of equal volume and temperature, which one of
these statements is true?
a. The pressure in the O2 container is greater than that in the N2 container.
b. There are more N2 molecules than O2 molecules.
c. There are equal amounts (in moles) of both gases.
d. The average kinetic energy of N2 molecules is greater than that of O2 molecules.
e. The pressures of both gases are the same.
Problem
105. Compressed-air tanks are often attached to water-well systems to relieve the strain on electrical water pumps.
These compressed-air tanks are normally pressurized to 20 psi. If the air were totally released from a 45 L
tank, what volume of air would be released at a normal pressure of 14.7 psi?
106. At a depth of 300 m in the ocean, the pressure is approximately 33 atm. If the air bladder of a certain deepwater fish is 6 mL at this depth, what will the volume of the air bladder become if the fish were raised to the
surface at 1 atm of pressure? What effect might this have on the fish?
107. A particular football has an internal volume of 2.25 L at an outdoor temperature of 35C. When the football
is brought indoors, the temperature in the football drops to 20C. What is the new volume of the football?
108. In an investigation to examine Charles’s law, a syringe is filled with 30 mL of air at a room temperature of
25C. If the syringe is placed in a water bath and the temperature is raised to 80C, what volume does the
syringe now read?
109. Hot air balloons are open containers that maintain the air inside at (very nearly) atmospheric pressure. When a
modern balloon’s propane burner has warmed the air inside from an average value of 21C to an average
value of 85C, find the final volume of each 10.00 L of air that was initially in the balloon.
110. Halogen lamp bulbs are made of quartz to withstand the high pressure that develops when they heat up to
temperatures of 1000C during operation. If a halogen bulb is filled with iodine vapour at 5.00 atm of
pressure, what will be the pressure in the bulb when it reaches its operating temperature, if room temperature
is 22C?
111. Non-alcoholic champagne is a carbonated beverage. Carbon dioxide is forced into the bottle at five times
atmospheric pressure. If the bottle is 750 mL in size, what volume of carbon dioxide would be released at an
atmospheric pressure of 99 kPa if the champagne were totally flat.
112. In order to launch a spud (potato) gun, air is compressed to a value of 10.0 mL. When the gun is fired and the
pressure is returned to an atmospheric pressure of 101 kPa, the volume of gas released is 130 mL. Calculate
the pressure of air before firing in the potato gun.
113. Ordinary incandescent light bulbs contain a tungsten filament which becomes white hot at a temperature of
2500C. These light bulbs are typically filled with inert argon gas at a low pressure of 5 mmHg (torr)
a. Describe what occurs at a molecular level as the light bulb is turned on.
b. If the initial temperature of the light bulb is 20.0C, to what pressure does the bulb rise when the light is
on? Report your answer in mmHg and kPa .
c. Why might the bulb be filled with argon as opposed to other common gases?
114. Perform the following temperature conversions.
a. 23.0°C to K
b. –52.00°C to K
c. 152 K to °C
d. 420 K to °C
115. When carbonating pop, equal amounts of pop and carbon dioxide are placed in the container. If the volume of
the pop bottle is 2.0 L, and the volume of gas collected was 6.8 L at 100.5 kPa, what pressure is the carbon
dioxide kept at in the pop bottle?
116. A 5.5 L balloon is completely filled with air indoors at a temperature of 21.0C. The balloon is taken out on a
cold winter day. If the final volume of the balloon is 4.5 L, what is the Celsius temperature outdoors?
117. The pressure in a can of pop is 350 kPa at a room temperature of 25C. The can is placed in a refrigerator and
the temperature drops to 5C. What is the new pressure in the can?
118. A propane barbeque tank is filled in the summer at 32C to a pressure of 2500 kPa. In the winter, what will
the pressure become if the temperature drops to –20C?
119. A fire extinguisher containing carbon dioxide has an operating pressure of 950 kPa and an operating volume
of 60 L. When the tank is completely discharged at 101 kPa, what volume would the carbon dioxide occupy?
120. A child’s toy beachball was played with during the day when the temperature was 25C. However, the ball
was left out overnight, and when observed in the morning, it appeared somewhat deflated. The temperature in
the morning had dropped to 3C.
a. Using diagrams, explain the observed deflation in the ball.
b. Calculate the volume of the ball at the reduced temperature if the initial volume of the ball was 3.4 L.
c. Noticing that the ball was deflated, the child had the ball reinflated to its normal size. The temperature
that day began to rise back to 25C. Discuss why might this be a problem.
121. Mount Logan is the highest mountain in Canada and is located within Kluane National Park and Reserve in
southwestern Yukon. Mount Logan rises to a height of 5959 m. The average temperature of Mt. Logan is –
27C.
a. Why is the pressure so much lower than standard atmospheric pressure?
b. A typical breath of air requires 0.5 L of air at 20?C to provide enough oxygen. How many breaths must
be taken to get the same volume of air at 20?C?
122. The air pressure in the middle ear is usually the same as the air pressure outside of the body. A tube called the
Eustachian tube connects the middle ear to the back of the nose and upper throat. Swallowing or yawning and
the resulting flow of air can be used to equalize air pressure. If the air tube is blocked and pressure cannot be
equalized, barotrauma can result, and the ear drum can rupture.
a. Explain why diving to depths of 3 m can result in barotrauma.
b. Why might barotrauma be a problem at higher altitudes?
123. Pop Rocks are a type of candy that pops when dissolved in a person’s mouth. The popping is a result of
trapped gas being released at less pressure in the mouth. If the average trapped bubble of gas in the Pop Rocks
has a volume of 0.15 mL at a pressure of 600 psi, calculate the volume of the gas released at an atmospheric
pressure of 102 kPa.
124. A gas tank containing oxygen used for classroom demonstrations has a volume of 3.00 L at a pressure of 1200
kPa. How many 250 mL round-bottom flasks can be filled with the oxygen in this tank, assuming that the
temperature is constant and atmospheric pressure is 100.0 kPa?
125. A sealed sandwich bag in the freezer contains a food item with 100.0 mL of air trapped in the bag at –25C.
The sandwich is removed from the freezer and placed on a counter at 32C.
a. Describe the changes that will take place with the air in the bag as it sits on the counter.
b. Determine the volume of the air in the bag at the new temperature.
126. The temperature of steam can be raised to very high temperatures. At these temperatures, when the steam is
released, it can be used to move an object. If 2.00 L of steam is at a pressure of 205 psi at 150C, calculate
the pressure of steam if the temperature is raised to 250C. Assume that the volume does not change.
127. A balloon was inflated in the summer at 35C to a volume of 25 L. The balloon was left in an outdoor shed.
When observed in the winter, the volume of the balloon had been reduced to 19 L. What was the temperature
of the shed in the winter, in degrees Celsius?
128. A container can withstand a maximum internal pressure of 8 atm. If the container is filled with a gas at 25C
and 99 kPa, at what temperature (in C) will the container explode?
129. The volume of a cylinder is 545 cm3 at a pressure of 1.2 atm. If the volume is reduced by 90 percent, what
pressure must have been exerted?
130. A tire is inflated in the winter to a pressure of 400 kPa at –22C. In the spring, the air temperature rises to
19C.
a. Calculate the tire pressure in the spring.
b. Tire manufacturers recommend that you check your tire pressure regularly. Explain this advice.
131. An air compressor used to fire nails into wood structures operates best up to a pressure of 120 psi. If the
compressor tank holds 55 L of air, what volume of air at 100.5 kPa must be compressed?
132. Examine the data presented in the table below.
Pressure (kPa)
100.0
200.0
300.0
400.0
Volume of Gas (mL)
35.0
17.5
5.0
a. Does this data support Boyle’s law? Give evidence to support your answer.
b. Predict the volume of the gas at a pressure of 400.0 kPa.
133. Examine the data presented in the table below.
Temperature (C)
20
30
40
50
Volume of Gas (mL)
250
259
266
a. Does this data support Boyle’s law? Give evidence to support your answer.
b. Predict the volume of the gas at 50C.
134. Hot air balloons operate on the principle that heated air is less dense than colder air. Using conditions that you
create, verify that this is true. The molar mass of dry air is 28.97 g/mol and the density of dry air is 1.29 g/L at
STP.
135. A sample of XH3(g) with a mass of 0.820 g occupies a volume of 550 mL at a pressure of 110 kPa and
28.5C.
a. Determine the molar mass of the compound XH3.
b. Identify the element X.
136. Acetylene, C2H2, an important gas for welding, can be produced in the laboratory by reacting calcium carbide
with water according to the equation:
CaC2(s) + 2H2O(l) → C2H2(g) + Ca(OH)2(aq)
a. During a reaction, 758 mL of acetylene was collected at a pressure of 740 mmHg and a temperature of
25C. What mass of acetylene was collected?
b. Assuming a complete reaction, what mass of calcium carbide was used up in the reaction?
137. Some commercial drain cleaners use a mixture of sodium hydroxide and aluminum powder. When the solid
mixture is poured into the drain and dissolves, a reaction ensues that produces hydrogen gas:
2NaOH(aq) + Al(s) + 6H2O(l) → 2NaAl(OH)4(aq) + 3H2(g)
Determine the volume of hydrogen gas produced when 4.00 g of aluminum reacts with excess sodium
hydroxide if the temperature is 40.0C and the pressure is 101 kPa.
138. Potassium metal reacts violently with water according to the following reaction:
2K(s) + 2H2O(l) → H2(g) + 2KOH(aq)
A 5.00 g sample of metal was reacted with water.
a. What volume of dry hydrogen gas would be produced at 102 kPa and 20C?
b. During one reaction, 545 mL of wet hydrogen gas was collected. If the gas was collected at 750 mmHg
and 31C, what mass of potassium was reacted?
c. After the reaction is over, evaporation of water will leave the solid KOH. What mass of NaOH can be
produced if the 870 mL of dry hydrogen gas is produced at 25C and 1.1 atm?
139. When Antoine Lavoisier was studying the nature of combustion reactions, he heated mercury(II) oxide to
obtain oxygen gas and liquid mercury. What volume of dry hydrogen gas would be collected by water
displacement if 1.05 kg of the oxide was heated and the gas was collected at SATP?
140. Carbon dioxide at high levels can cause death. One method of removing carbon dioxide from the air of
enclosed compartments involves the reaction of carbon dioxide with sodium hydroxide:
2NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l)
What mass of sodium hydroxide is required to remove all the carbon dioxide in the air over a 12 h period if
the volume of CO2 produced is 0.75 L per minute at a temperature of 25C and a pressure of 102 kPa?
141. Tetrachloroethylene is a powerful liquid solvent that has a high vapour pressure and evaporates easily. It has
been used to decaffeinate coffee, as paint thinner, and as a solvent to clean computer hardware. It has a
boiling point of 121C When the chemical is vaporized at 140C at 120 kPa, it has a gaseous density of 5.79
g/L.
a. Calculate the molar mass of the compound.
b. If the empirical formula of the compound is CCl2, determine the molecular formula of the compound.
142. A relatively recent invention offered to the Canadian public is propane-powered mosquito traps. This
invention utilizes the combustion of propane to attract mosquitoes.
a. Write the balanced equation for the combustion reaction for propane (C3H8) in the presence of oxygen.
b. A typical barbeque tank may contain 7.3 kg of propane. Calculate the volume of carbon dioxide that is
released by the tank during combustion if the air temperature is 42C and the pressure is 100.8 kPa.
143. Antacids often contain carbonates that are used to reduce excess stomach acid. Carbonates such as calcium
carbonate are often manufactured in tablet form and are available over the counter. The reaction with
stomach acid is a neutralization reaction:
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(g)
What volume of carbon dioxide gas would be generated if a person consumed 15 tablets, each with a mass of
500.0 mg, if the temperature is 37C and the pressure is 102 kPa? Assume that the tablets all react.
144. An organic compound used in the production of sweet-smelling perfumes was isolated and examined. It was
found to contain the composition of 54.52 % carbon, 9.17% hydrogen, and the remaining percentage oxygen.
In a second procedure, it was found that 1.76 g of the volatile liquid was able to fill a 288 mL Erlenmeyer
flask at 99.8 kPa and 80C.
a. Determine the empirical formula of the compound.
b. Determine the molar mass of the compound.
c. Determine the molecular formula of the compound.
145. Ammonium sulfate, an important fertilizer, can be prepared by the reaction of ammonia with sulfuric acid,
according to the following balanced equation:
2NH3(g) + H2SO4 → (NH4)2SO4(aq)
Calculate the volume of NH3 (in litres) needed at 31°C and 2500 kPa to react
with 1500 g of H2SO4.
146. A small bubble rises from the bottom of a lake, where the temperature and pressure are 4°C and 3.0 atm, to
the water‘s surface, where the temperature is 25°C and the pressure is 0.95 atm. Calculate the final volume of
the bubble if its initial volume was 2.1 mL.
147. A sample of ammonia used as a refrigerant is circulated through a series of pipes for refrigeration. If the gas
occupies 450 cm3 at a pressure of 140 psi and a temperature of 12C, what volume of gas will be released if
there is break in the line when the external temperature is 32C and the external pressure is 101 kPa?
148. Propane gas stored in a 200 L tank at –15C and a pressure of 110 atm is being used to fuel a gas fireplace.
The gas fireplace consumes 350 L of gas a day at a burning temperature of 25C and 101 kPa pressure. How
many days will the propane supply last?
149. Suppose a car engine cylinder has a volume of 575 mL when the gas is injected. The gas has a temperature of
22C and a pressure of 97.0 kPa. At the time of firing the cylinder, the volume has changed to 55.1 mL and
the gas is at a temperature of 1360C. What is the pressure of the gas at this time?
150. A sample of refrigeration gas has a volume of 405 mL at a pressure of 1.50 atm and a temperature of 28C.
The gas was compressed into a volume of 130 mL with a pressure of 3.8 atm. What temperature in degrees
Celsius did the gas change to?
151. A gas filled weather balloon has a volume of 75.0 L and is released at sea level where the temperature is
30.0C and the pressure is 765 mmHg. The balloon can expand to a maximum volume of 900 L. When the
balloon rises to certain altitude, the temperature is –5C and the pressure is 50 mmHg. Will the balloon reach
its maximum volume?
152. The dirigible Hindenberg had a volume of 3.7  106 m3 of hydrogen in its inflatable gas bags. What mass
would this amount of gas weigh at an atmospheric pressure of 1.2 atm and a temperature of 10C?
153. The liquid oxygen tank of the NASA shuttle has volume of 5.5  105 L at a pressure of 150 kPa and
temperature of –183C.
a. What mass of oxygen is present at this temperature and pressure?
b. If all the oxygen gas were to be released at an average temperature of SATP, what volume would it
occupy?
c. When the shuttle is launched, liquid oxygen is used at a maximum rate of 6.6  104 L/min. Under these
conditions, how long does it take to exhaust the oxygen tank?
154. Calculate the ideal gas constant using atmospheres for the pressure unit.
155. Calculate the ideal gas constant using mmHg for the pressure unit.
156. If the density of chlorine gas is 3.21 g/L, calculate the molar volume at STP.
157. If the density of carbon monoxide gas is 1.25 g/L, calculate the molar volume at STP.
158. Air has an average molar mass of 28.8 g. An air compressor has a pressure gauge reading of 8.5 atm at 23C
air temperature. The volume of the compressor is 28 L. What is the mass of the air alone in the compressor?
159. Calculate the density of carbon dioxide gas at a temperature of –45C and an air pressure of 99.5 kPa.
160. Calculate the molar mass of a compound if 10.05 g of a gas occupies 1.20 L at 29.2C and 1.1 atm.
161. A dry ice bomb is a demonstration device that relies on the sublimation of carbon dioxide. A mass of dry ice
is placed inside a sealed plastic container with a lid that is snapped shut. The dry ice is allowed to sublimate
and eventually the lid of the container is “fired” across a room.
a. Describe the changes that would occur inside the container as the dry ice sublimates. Explain why the
bottle cap is propelled from the lid.
b. A 50.0 g sample of dry ice was placed in a 2.0 L bottle at a temperature of 25C. Assuming no
temperature change, calculate the pressure that would develop inside the sealed container when all the
solid carbon dioxide has sublimated..
162. Calculate the molar mass of a compound if 5.88 g of a gas occupies 0.98 L at 31C and 104 kPa.
163. A gas cylinder contains 50.0 L of the gas argon when it is full. If the cylinder was at an internal pressure of
1500 kPa and 25C, how many molecules of argon gas were present in the container?
164. A certain organic molecule contains carbon, hydrogen, and oxygen. This particular compound has a most
putrid odour. Analysis of the compound reveals that it contains 54.5 % carbon ,31.8 % nitrogen, and the
remainder hydrogen by mass. A sample of the compound weighing 0.826 g at 27C and 103 kPa fills a 226
mL container.
a. Determine the empirical formula from the data above.
b. Determine the molar mass of the compound.
c. Given your answers to (a) and (b), determine the molecular formula of the compound.
165. A balloon containing hydrogen gas has a volume of 3.5 L. The mass of the hydrogen in the balloon is 0.326 g.
If the pressure of the gas is 120 kPa, what is the temperature of the gas in degrees Celsius?
166. In an attempt to determine the molar mass of air, the mass of an empty 60 mL syringe was measured. The
plunger was then pulled to the 60.0 mL mark and the mass of the syringe was measured again. The data are
presented below.
Item Measured
Measurement
Mass empty syringe (g)
45.780
Mass syringe with air (g)
45.850
Air temperature (C)
22.3
Air pressure (kPa)
100.4
a. Based on the data above, determine the molar mass of air.
b. Would the molar mass of air vary with the temperature? Explain.
c. If the air were humid, would this affect the molar mass? Explain..
167. The head of a match contains the chemical diphosphorus trisulfide. When this chemical undergoes friction it
ignites and burns according to the equation given below:
P2S3(s) + 11/2 O2(g) → P2O5(g) + 3SO2(g)
What mass of P2S3 would produce 310 mL of sulfur dioxide gas (SO2) at a pressure of 101.2 kPa and a
temperature of 37C?
168. In the presence of a manganese(IV) oxide catalyst, hydrogen peroxide decomposes to form water and oxygen
gas:
a. Write a balanced equation for this reaction.
b. What volume of oxygen gas would be produced when 500 mL of 3 M hydrogen peroxide solution
decomposes at 35C and 99 kPa?
169. One method of producing ammonia gas involves the reaction of ammonium chloride with sodium hydroxide
according to the following equation:
NH4Cl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) + NH3(g)
Suppose 98.0 mL of ammonia gas was collected using water displacement.
a. If the gas were collected at 20.0C and 780 mmHg, determine the amount (in moles) of sodium hydroxide
that must have reacted.
b. If the volume of solution when reacted was 100.0 mL, determine the concentration of NaOH at the start
of the reaction.
170. Kilauea Volcano on the Island of Hawaii emits about 2000 tons of sulfur dioxide (SO2) gas each day during
periods of sustained eruption.
a. Calculate the volume of SO2 (in litres) emitted over an entire year if the average temperature of the gas is
40C and the pressure is 101 kPa.
b. Local winds can often drive SO2 emissions from the volcano across populated areas on the island.
Speculate as to the potential dangers or health effects of such distribution.
171. A commercial refrigeration unit accidentally releases 1550 L of ammonia (NH3) gas
at 15C and 99 kPa. Determine the number of molecules released under these conditions.
172. A acetylene (C2H2) tank used for welding has a mass of 54 kg. Calculate the pressure of the gas in the tank if
the volume of the tank is 200.0 L at 18C.
fsf
Answer Section
MULTIPLE CHOICE
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11.1 | 11.2 | 11.3
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U | T/I
K/U
K/U | T/I
T/I
T/I
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K/U | T/I
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11.1 | 11.2 | 11.3
T/I
T/I
K/U
K/U
K/U
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K/U
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T/I
K/U
T/I
K/U
PTS: 1
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TOP: 11.3
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TOP: 11.1
MSC: T/I
MSC: K/U
MSC: K/U
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ANS:
ANS:
ANS:
ANS:
D
E
D
D
D
C
C
E
B
C
A
B
C
E
C
B
E
B
C
B
A
B
B
B
A
C
T/I
E
E
D
D
B
A
E
D
C
D
B
E
E
D
B
E
D
E
A
A
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
11.3
MSC:
11.3
MSC:
11.1
MSC:
11.3
MSC:
11.1
MSC:
11.3
MSC:
11.2
MSC:
11.3
MSC:
11.1
MSC:
11.2
MSC:
11.3
MSC:
11.3
MSC:
11.1
MSC:
11.2 | 11.3
MSC:
11.1
MSC:
11.2
MSC:
11.3
MSC:
11.1
MSC:
11.1
MSC:
11.1 | 11.3
MSC:
11.1
MSC:
11.1
MSC:
11.3
MSC:
11.1 | 11.2
MSC:
11.3
MSC:
11.1 | 11.2 | 11.3
K/U
K/U
K/U
K/U
K/U
T/I
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U
T/I
K/U
T/I
K/U
T/I
T/I
T/I
K/U
K/U
T/I
T/I
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
11.2
11.1
11.1 | 11.3
11.1
11.2
11.1
12.1
12.2
12.2
12.2
12.2
12.1
12.2
12.2
12.2
12.2
12.2
12.2
12.2
12.2
K/U
K/U
K/U
K/U
K/U
K/U
K/U
T/I
K/U
T/I
K/U
K/U
K/U
T/I
T/I
K/U
K/U
K/U
K/U
K/U
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
85.
86.
87.
88.
89.
90.
91.
92.
93.
94.
95.
96.
97.
98.
99.
100.
101.
102.
103.
104.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
C
E
B
E
D
B
C
C
E
B
C
D
D
E
B
C
B
B
E
A
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
TOP:
TOP:
TOP:
TOP:
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TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
TOP:
12.2
12.1
12.1
12.1
12.1
12.1
12.1
12.1
12.2
12.2
12.1
12.1
12.2
12.1
12.1
12.1
12.3
12.3
12.2
12.2
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
MSC:
K/U
K/U
K/U
K/U
K/U
T/I
T/I
K/U
T/I
T/I
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U
PROBLEM
105. ANS:
PTS: 5
106. ANS:
TOP: 11.3
MSC: T/I
At this volume, it is likely that the air bladder would rupture and the fish would be killed.
PTS: 5
TOP: 11.2
107. ANS:
T1 = 35C + 273 = 308 K
T2 = 20C + 273 = 290 K
V1 = 2.25 L
MSC: T/I
PTS: 5
TOP: 11.3
108. ANS:
T1 = 25C + 273 = 298 K
MSC: T/I
T2 = 80C + 273 = 353 K
V1= 30 mL
PTS: 5
TOP: 11.3
109. ANS:
T1 = 21C + 273 = 294 K
MSC: T/I
T2 = 85C + 273 = 358 K
V1= 10.00 L
PTS: 5
TOP: 11.3
110. ANS:
T1 = 22C + 273 = 295 K
T2 = 1000C + 273 = 1273 K
MSC: T/I
PTS: 5
TOP: 11.3
111. ANS:
P1 = 5  99 kPa = 495 kPa
MSC: T/I
P2 = 99 kPa
V1 = 750 mL
PTS: 5
112. ANS:
P1 = 101 kPa
TOP: 11.2
MSC: T/I
V1 = 130 mL
V2 = 10.0 mL
PTS: 5
TOP: 11.2
MSC: T/I
113. ANS:
a. The filament heats up, causing the gas to heat up. The molecules of gas move faster, striking the surface
of the bulb more frequently. This means that the internal pressure of the bulb increases.
b. T1 = 2500C + 273 = 2773 K
T2 = 20.0C + 273 = 293 K
P1= 5 mmHg
c. Argon is inert and would not react with the filament.
PTS: 5
TOP: 11.3
114. ANS:
a. 23C + 273 = 296 K
MSC: T/I | A
b. –52.00C + 273 = 221 K
c. 152 K – 273 = –121C
d. 420 K – 273 = 147C
PTS: 5
115. ANS:
TOP: 11.3
MSC: T/I
PTS: 5
116. ANS:
TOP: 11.2
MSC: T/I
T1 = 21C + 273 = 294 K
V1= 5.5 L
V2 = 4.5 L
PTS: 5
TOP: 11.3
117. ANS:
T1 = 25C + 273 = 298 K
MSC: T/I
T2 = 5C + 273 = 278 K
P1 = 350 kPa
PTS: 5
TOP: 11.3
118. ANS:
T1 = 32C + 273 = 305 K
MSC: T/I
T2 = –20C + 273 = 253 K
P1 = 2500 kPa
PTS: 5
119. ANS:
P1 = 950 kPa
TOP: 11.3
MSC: T/I
P2 = 101 kPa
V1 = 60 L
PTS: 5
TOP: 11.2
MSC: T/I
120. ANS:
a. Molecules are moving slower as temperature is reduced. This results in decreased volume.
b. T1 = 25C + 273 = 298 K
T2 = 3C + 273 = 276 K
V1 = 3.4L
c. As temperature rises, particles move faster and volume increases. This may cause the ball to burst.
PTS: 5
TOP: 11.1 | 11.3
MSC: C | T/I
121. ANS:
a. Atmospheric pressure decreases with increasing elevation, or altitude. At higher altitudes, there are less
gaseous particles per given volume, and thus the pressure is reduced.
b. T1 = –27C + 273 = 246 K
T2 = 20C + 273 = 293 K
V1 = 0.5 L
You would need to take an extra quarter breath every time.
PTS: 5
TOP: 11.2
MSC: T/I
122. ANS:
a. Increased pressure on the inner ear can cause the rupture to take place (Boyle’s law).
b. There is a decrease in air pressure, and if pressure cannot be equalized, the pressure in the ear will push
outward and burst the ear drum.
PTS: 5
123. ANS:
P1 = 600 psi
V1 = 0.15 mL
P2 = 102 kPa
TOP: 11.1 | 11.2
MSC: T/I | C | A
PTS: 5
124. ANS:
P1 = 1200 kPa
TOP: 11.2
MSC: T/I
V1 = 3.00 L
P2 = 100.0 kPa
PTS: 5
TOP: 11.2
MSC: T/I
125. ANS:
a. As the temperature rises, the molecules of gas will begin to move faster and farther apart. This will result
in the sandwich bag increasing in volume.
b. T1 = –25C + 273 = 248 K
T2 = 32C + 273 = 305 K
V1 = 100 mL
PTS: 5
TOP: 11.3
126. ANS:
T1 = 150C + 273 = 423 K
T2 = –20C + 273 = 523 K
P1 = 200 psi
MSC: T/I
PTS: 5
TOP: 11.3
127. ANS:
T1 = 35C + 273 = 308K
MSC: T/I
V1 = 25 L
V2 = 19 L
T2 = 234 K – 273 = –39C
PTS: 5
TOP: 11.3
128. ANS:
T1 = 25C + 273 = 298 K
MSC: T/I
P1 = 8 atm
P2 = 99.5 kPa
T2 = 2430 K – 273 = 2160C
PTS: 5
129. ANS:
TOP: 11.3
MSC: T/I
P1 = 1.2 atm
V1 = 545 cm3
100% – 90% = 10%
V2 = 545 cm3  0.1 = 54.5 cm3
PTS: 5
TOP: 11.2
130. ANS:
a. T1 = –22C + 273 = 251 K
T2 = 19C + 273 = 292 K
P1 = 405 kPa
MSC: T/I
b. Temperature variations during the change in seasons will effect tire pressure. If the tire pressure exceeds
the recommendations of the manufacturer, it is possible that the air may leak from the tire, or the tire may
explode.
PTS: 5
131. ANS:
P1 = 120 psi
TOP: 11.3
MSC: T/I
TOP: 11.2
MSC: T/I
P2 = 100.5 kPa
V1 = 55 L
PTS: 5
132. ANS:
a. To answer this question, students could graph the data. Alternatively, they could multiply temperature
versus pressure and see if a constant resulted.
100.0 kPa  35.0 mL = 3500
200.0 kPa  17.5 mL = 3500
b. To determine the unknown quantity:
PTS: 5
TOP: 11.2
MSC: A | C | T/I
133. ANS:
a. To answer this question, students could graph the data. Alternatively, they could convert temperatures to
degrees Kelvin and assess if volume divided by the Kelvin temperature is a constant.
b. To predict the value:
PTS: 5
134. ANS:
1 mol = 28.97 g
TOP: 11.3
D = 1.29 g/L
T = 0C
P = 101.3 kPa
At 0C, 1 mol occupies 22.4 L
At 25C, for example:
1 mol = 24.46 L
MSC: T/I | A | C
To calculate density:
Clearly, the density decreases with increasing temperature.
PTS: 5
135. ANS:
a. V = 0.550 L
TOP: 12.2
MSC: T/I
T = 28.5C + 273 = 301.5 K
P = 110 kPa
b. XH3
3  1.01 g/mol = 3.03 g/mol
34.02 g/mol – 3.03 g/mol = 30.99 g/mol
The element that fits this description is phosphorus.
The element X is phosphorus.
PTS: 5
136. ANS:
a. V = 0.758 L
TOP: 12.2
MSC: T/I
T = 25C + 273 = 298 K
1 mol C2H2 = (12.01  2 + 1.01  2) = 26.04 g
b. 1 mol CaC2 = (40.08 + 12.01  2) = 64.10 g
PTS: 5
137. ANS:
P = 101 kPa
TOP: 12.2
T = 40C + 273 = 313 K
MSC: T/I
1 mol Al = 26.98 g
PTS: 5
138. ANS:
a. P = 102 kPa
TOP: 12.2
MSC: T/I
= 2.33 kPa
= 102 kPa – 2.33 kPa = 99.67 kPa
T = 20C + 273 = 293 K
1 mol K = 39.10 g
b.
V = 545 mL = 0.545 L
T = 31C + 273 = 304 K
c.
= 3.36 kPa
= 111.43 kPa – 3.36 kPa = 108.07 kPa
1 mol NaOH = (22.99 + 16.00 + 1.01) g = 40.00 g
V = 870 mL = 0.870 L
T = 25C + 273 = 298 K
PTS: 5
139. ANS:
Reaction is:
TOP: 12.2
MSC: T/I
2HgO(s) → 2Hg(l) + O2(g)
1.05 kg = 1050 g
P = 100.0 kPa
= 3.36 kPa
= 100.0 kPa – 3.36 kPa = 96.64 kPa
T = 25C + 273 = 298 K
1 mol HgO = (200.59 + 16.00) = 216.59 g
PTS: 5
TOP: 12.2
MSC: T/I
140. ANS:
1 mol NaOH = (22.99 + 16.00 + 1.01) g = 40.00 g
T = 25C + 273 = 298 K
P = 102 kPa
PTS: 5
141. ANS:
a. V = 1.00 L
TOP: 12.2
MSC: T/I
T = 140C + 273 = 413 K
l
b. 1 mol CCl2 = (12.01 + 35.45  2) = 82.91 g
2  CCl2 = C2Cl4
The chemical formula is C2Cl4.
PTS: 5
TOP: 12.2
MSC: T/I
142. ANS:
a. C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
b. 1 mol C3H8 = (12.01  3 + 1.01  8) = 44.11 g
7.3 kg = 7300 g
P = 100.8 kPa
T = 42C + 273 = 315 K
PTS: 5
TOP: 12.2
MSC: T/I
143. ANS:
1 mol CaCO3 = (40.01 + 12.01 + 16.00  3) = 100.02 g
500.0 mg = 0.5000 g
P = 102 kPa
T = 37C + 273 = 310K
PTS: 5
144. ANS:
a. Assume 100 g.
TOP: 12.2
MSC: T/I
empirical formula is C2H4O1
b. V = 0.288 L
T = 80C + 273 = 353 K
c. 1 mol C2H4O = (12.01  2 + 1.01  4 + 16.00  1) = 44.06 g
4  C2H4O = C8H16O4
PTS: 5
TOP: 12.2
MSC: T/I
145. ANS:
1 mol H2SO4 = (1.01  2 + 32.07 + 16.00  4) = 98.09 g
P = 2500 kPa
T = 31°C + 273 = 304 K
PTS: 5
146. ANS:
V1 = 2.1 mL
TOP: 12.2
MSC: T/I
T1 = 4°C + 273 = 287 K
P1 = 3.0 atm
T2 = 25°C + 273 = 298 K
P2 = 0.95 atm
PTS: 5
147. ANS:
V1 = 450 cm3
TOP: 12.1
MSC: T/I
T1 = 12C + 273 = 285 K
P1 = 140 psi
T2 = 32C + 273 = 305 K
PTS: 5
148. ANS:
V1 = 200 L
TOP: 12.1
T1 = –15C + 273 = 258
P1 = 101 atm
T2 = 2C5 + 273 = 298 K
P2 = 101 kPa
MSC: T/I
PTS: 5
149. ANS:
V1 = 575 mL
TOP: 12.1
MSC: A | T/I
T1 = 22C + 273 = 295 K
P1 = 97.0 kPa
T2 = 1360C + 273 = 1633 K
V2 = 55.1 mL
PTS: 5
150. ANS:
V1 = 405 mL
TOP: 12.1
MSC: T/I
T1 = 28C + 273 = 301 K
P1 = 1.50 atm
P2 = 3.8 atm
V2 = 130 mL
245 K – 273 K = –28 K
PTS: 5
151. ANS:
V1 = 75.0 L
TOP: 12.1
MSC: T/I
T1 = 30 + 273 = 303K
P1 = 765 mmHg
T2 = -5 + 273 = 268K
P2 = 50 mmHg
The balloon will reach its maximum value and is likely to explode
PTS: 5
152. ANS:
V = 3.7  106 m3
TOP: 12.1
T = 10C + 273 = 373K
MSC: T/I
1 m3 = 1000 L
PTS: 5
153. ANS:
a. V = 5.5  106 L
TOP: 12.2
MSC: T/I
P = 105 kPa
T = –183C + 273 = 90 K
b.
c.
PTS: 5
154. ANS:
1 mol = 22.4 L
T = 273.15 K
P = 1 atm
TOP: 12.2
MSC: T/I
PTS: 5
155. ANS:
1 mol = 22.4 L
TOP: 12.2
MSC: T/I
T = 273.15 K
P = 760 mmHg
PTS: 5
TOP: 12.2
156. ANS:
1 mol Cl2 = (35.45 g  2) = 70.90 g
MSC: T/I
PTS: 5
TOP: 12.2
157. ANS:
1 mol CO = (12.01 + 16.00) = 28.01 g
MSC: T/I
PTS: 5
158. ANS:
1 mol = 28.8 g
MSC: T/I
TOP: 12.2
V = 28 L
T = 23C + 273 = 296 K
PTS: 5
TOP: 12.2
159. ANS:
1 mol = (12.01 + 2  16.00) g = 44.01 g
V=1L
MSC: T/I
T = –45C + 273 = 228 K
P = 99.5 kPa
The density of carbon dioxide gas under these conditions is 2.31 g/L.
PTS: 5
160. ANS:
V = 1.20 L
TOP: 12.2
MSC: T/I
T = 29.2C + 273 = 302.2 K
PTS: 5
TOP: 12.2
MSC: T/I
161. ANS:
a. As the solid carbon dioxide sublimates, gas is formed. The pressure inside the bottle will begin to increase
as more carbon dioxide gas is produced. This will cause the bottle to swell and eventually explode.
b. 1 mol = (12.01 + 2  16.00) g = 44.01 g
V=2L
T = 25C + 273 = 298 K
PTS: 5
162. ANS:
V = 0.98 L
TOP: 12.1 | 12.2
T = 31C + 273 = 304K
MSC: C | T/I
PTS: 5
163. ANS:
V = 50.0 L
TOP: 12.2
MSC: T/I
T = 25C + 273 = 298 K
PTS: 5
164. ANS:
a. Assume 100 g.
TOP: 12.2
MSC: T/I
empirical formula is C2H6N1
b. V = 0.226 L
T = 27C + 273 = 300 K
c. 1 mol C2H6N = (12.01  2 + 1.01  6 + 14.01  1) = 44.09 g
2  C2H6N = C4H12N2
PTS: 5
165. ANS:
V = 3.5 L
TOP: 12.2
MSC: A | T/I
P = 120 kPa
1 mol H2 = (1.01  2) = 2.02 g
T = 313 K – 273 = 40C
PTS: 5
TOP: 12.2
MSC: T/I
166. ANS:
a. mass of air = 45.850 g – 45.780 g = 0.07 g
P = 100.4 kPa
T = 22.3C + 273.2 = 295.5 K
b. As the temperature is raised, air particles move faster and farther apart, so the density would be expected
to decrease. If the temperature is lowered, gas molecules come closer together, so it would be expected
that the density would increase.
c. If the air was humid, more water molecules would be in the air. This would have the effect of making air
“heavy,” so it would increase the molar mass of the air.
PTS: 5
167. ANS:
V = 0.31 L
TOP: 12.2
MSC: A | T/I
P = 101.2 kPa
T = 37C + 273 = 310 K
1 mol P2S3 = (30.97  2 + 32.07  3) = 158.15 g
PTS: 5
TOP: 12.2
168. ANS:
a. 2H2O2(l) → 2H2O(l) + O2(g)
MSC: T/I
b. V = 0.5 L
C=3M
T = 35 + 273 = 308 K
P = 99 kPa
PTS: 5
169. ANS:
a. V = 0.098 L
TOP: 12.2
MSC: T/I
T = 20.0C + 273 = 293 K
b.
PTS: 5
TOP: 12.2
170. ANS:
a. T = 40C + 273 = 313 K
P = 101 kPa
MSC: T/I
1 mol SO2 = (32.07 + 16.00  2) = 64.07 g
1 tonne = 1  106g
b. Sulfur dioxide is a known pollutant and is part of the AQHI. It is also a principal gas involved in causing
acid rain. It is likely to aggravate existing health conditions and cause breathing difficulties.
PTS: 5
TOP: 12.2 | 12.3
171. ANS:
T = 15C + 273 = 288 K
MSC: A | T/I
V = 1550 L
P = 99 kPa
PTS: 5
TOP: 12.2
172. ANS:
T = 18C + 273 = 291 K
MSC: T/I
V = 200.0 L
1 mol C2H2 = (12.01  2 + 1.01  2) = 26.04 g
1 kg = 1000 g
PTS: 5
TOP: 12.2
MSC: T/I