The partial pressure of carbon dioxide varies with seasons. Would you expect the partial pressure in the Northern Hemisphere to be higher in the summer or winter? Explain.

When ammonium nitrite $\left(\mathrm{NH}_4 \mathrm{NO}_2\right)$ is heated, it decomposes to give nitrogen gas. This property is used to inflate some tennis balls.
(a) Write a balanced equation for the reaction.
(b) Calculate the quantity (in grams) of $\mathrm{NH}_4 \mathrm{NO}_2$ needed to inflate a tennis ball to a volume of $86.2 \mathrm{~mL}$ at $1.20 \mathrm{~atm}$ and $22^{\circ} \mathrm{C}$.

The empirical formula of a compound is $\mathrm{CH}$. At $200^{\circ} \mathrm{C}, 0.145 \mathrm{~g}$ of this compound occupies $97.2 \mathrm{~mL}$ at a pressure of $0.74 \mathrm{~atm}$. What is the molecular formula of the compound?

Nitroglycerin, an explosive, decomposes according to the equation

$$\begin{aligned} & 4 \mathrm{C}_3 \mathrm{H}_5\left(\mathrm{NO}_3\right)_3(s) \longrightarrow \\ & 12 \mathrm{CO}_2(g)+10 \mathrm{H}_2 \mathrm{O}(g)+6 \mathrm{~N}_2(g)+\mathrm{O}_2(g) \end{aligned}$$

Calculate the total volume of gases produced when collected at $1.2 \mathrm{~atm}$ and $25^{\circ} \mathrm{C}$ from $2.6 \times 10^2 \mathrm{~g}$ of nitroglycerin. What are the partial pressures of the gases under these conditions?

Discuss the following phenomena in terms of the gas laws: (a) the pressure in an automobile tire increasing on a hot day, (b) the "popping" of a paper bag, (c) the expansion of a weather balloon as it rises in the air, (d) the loud noise heard when a lightbulb shatters.

At $27^{\circ} \mathrm{C}, 10.0$ moles of a gas in a $1.50$ $\mathrm{-L}$ container exert a pressure of $130 \mathrm{~atm}$. Is this an ideal gas?

The temperature of a real gas that is allowed to expand into a vacuum usually drops. Explain.

Write the van der Waals equation for a real gas. Explain clearly the meaning of the corrective terms for pressure and volume.

Under what set of conditions would a gas be expected to behave most ideally? (a) High temperature and low pressure, (b) high temperature and high pressure, (c) low temperature and high pressure, (d) low temperature and low pressure.

Give two pieces of evidence to show that gases do not behave ideally under all conditions.

At a certain temperature the speeds of six gaseous molecules in a container are $2.0 \mathrm{~m} / \mathrm{s}, 2.2 \mathrm{~m} / \mathrm{s}, 2.6 \mathrm{~m} / \mathrm{s}$, $2.7 \mathrm{~m} / \mathrm{s}, 3.3 \mathrm{~m} / \mathrm{s}$, and $3.5 \mathrm{~m} / \mathrm{s}$. Calculate the rootmean-square speed and the average speed of the molecules. These two average values are close to each other, but the root-mean-square value is always the larger of the two. Why?

The average distance traveled by a molecule between successive collisions is called mean free path. For a given amount of a gas, how does the mean free path of a gas depend on (a) density, (b) temperature at constant volume, (c) pressure at constant temperature, (d) volume at constant temperature, and (e) size of the atoms?

The temperature in the stratosphere is $-23^{\circ} \mathrm{C}$. Calculate the root-mean-square speeds of $\mathrm{N}_2, \mathrm{O}_2$, and $\mathrm{O}_3$ molecules in this region.

Compare the root-mean-square speeds of $\mathrm{O}_2$ and $\mathrm{UF}_6$ at $65^{\circ} \mathrm{C}$.