9.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law

Boyle, Charles, and Avogadro relationships combined into PV = nRT, then solved for whichever property is unknown as conditions change.

Chemistry 2e, 9.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law

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13 exercises

9.2 Exercise 2

Explain how the volume of the bubbles exhausted by a scuba diver (the figure) change as they rise to the surface, assuming that they remain intact.

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9.2 Exercise 4

An alternate way to state Avogadro’s law is “All other things being equal, the number of molecules in a gas is directly proportional to the volume of the gas.” (a) What is the meaning of the term “directly proportional?” (b) What are the “other things” that must be equal?

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9.2 Exercise 6

How would the graph in the figure change if the number of moles of gas in the sample used to determine the curve were doubled?

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9.2 Exercise 8

Determine the volume of 1 mol of CH₄ gas at 150 K and 1 atm, using the figure.

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9.2 Exercise 10

A spray can is used until it is empty except for the propellant gas, which has a pressure of 1344 torr at 23 °C. If the can is thrown into a fire (T = 475 °C), what will be the pressure in the hot can?

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9.2 Exercise 12

A 2.50-L volume of hydrogen measured at –196 °C is warmed to 100 °C. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.

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9.2 Exercise 16

How many moles of gaseous boron trifluoride, BF₃, are contained in a 4.3410-L bulb at 788.0 K if the pressure is 1.220 atm? How many grams of BF₃?

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9.2 Exercise 18

How many grams of gas are present in each of the following cases?

(a) 0.100 L of CO₂ at 307 torr and 26 °C

(b) 8.75 L of C₂H₄, at 378.3 kPa and 483 K

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9.2 Exercise 20

A cylinder of medical oxygen has a volume of 35.4 L, and contains O₂ at a pressure of 151 atm and a temperature of 25 °C. What volume of O₂ does this correspond to at normal body conditions, that is, 1 atm and 37 °C?

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9.2 Exercise 22

A 20.0-L cylinder containing 11.34 kg of butane, C₄H₁₀, was opened to the atmosphere. Calculate the mass of the gas remaining in the cylinder if it were opened and the gas escaped until the pressure in the cylinder was equal to the atmospheric pressure, 0.983 atm, and a temperature of 27 °C.

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9.2 Exercise 26

The effect of chlorofluorocarbons (such as CCl₂F₂) on the depletion of the ozone layer is well known. The use of substitutes, such as CH₃CH₂F(g), for the chlorofluorocarbons, has largely corrected the problem. Calculate the volume occupied by 10.0 g of each of these compounds at STP:

(a) CCl₂F₂(g)

(b) CH₃CH₂F(g)

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9.2 Exercise 28

A balloon with a volume of 100.21 L at 21 °C and 0.981 atm is released and just barely clears the top of Mount Crumpit in British Columbia. If the final volume of the balloon is 144.53 L at a temperature of 5.24 °C, what is the pressure experienced by the balloon as it clears Mount Crumpit?

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9.2 Exercise 30

If the volume of a fixed amount of a gas is tripled at constant temperature, what happens to the pressure?

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