Use the kinetic molecular theory to draw a molecular-level picture of a gas. Briefly describe the motion of the gas particles.

When do real gases behave as ideal gases?

When water is subjected to an electric current, it decomposes to hydrogen and oxygen gas. If $1.00 \mathrm{~g}$ of water is decomposed at $1.00 \mathrm{~atm}$ and $25^{\circ} \mathrm{C}$, what volume of oxygen gas is collected?

A $1.50 \mathrm{~L}$ sample of neon gas at $1.10 \mathrm{~atm}$ and $25^{\circ} \mathrm{C}$ is heated to $45^{\circ} \mathrm{C}$. The neon gas is then subjected to a pressure of $1.50 \mathrm{~atm}$. Determine the new volume of the neon gas.

Describe a simple mercury barometer. How is such a barometer used to measure the pressure of the atmosphere ?

What will the volume of the sample become if $459 \mathrm{~mL}$ of an ideal gas at $27^{\circ} \mathrm{C}$ and $1.05 \mathrm{~atm}$ is cooled to $15^{\circ} \mathrm{C}$ and $0.997 \mathrm{~atm}$ ?

Suppose two $200.0$-L tanks are to be filled separately with the gases helium and hydrogen. What mass of each gas is needed to produce a pressure of $135 \mathrm{~atm}$ in its respective tank at $24^{\circ} \mathrm{C}$ ?

Consider a mixture of equal masses of helium and hydrogen gases in a steel container. Which gas exerts the greater partial pressure, and by what factor?

A. The helium gas exerts about twice as much pressure as the hydrogen gas.
B. The helium gas exerts about four times as much pressure as the hydrogen gas.
C. The hydrogen gas exerts about twice as much pressure as the helium gas.
D. The helium gas exerts about the same pressure as the hydrogen gas.

Determine the pressure in a $125-\mathrm{L}$ tank containing $56.2\mathrm{~kg}$ of oxygen gas at $21^{\circ} \mathrm{C}$.

In Figure $13.8$ oxygen gas is being collected over water. Assume this experiment is being done at $25^{\circ} \mathrm{C}$. Write an equation for it, and find the pressure of the oxygen gas (assume the pressure in the bottle is $P_{\mathrm{T}}$ ).

At what temperature does $16.3 \mathrm{~g}$ of nitrogen gas have a pressure of $1.25 \mathrm{~atm}$ in a $25.0-\mathrm{L}$ tank?

Given each of the following sets of values for an ideal gas, calculate the unknown quantity. a. $P=782 \mathrm{~mm} \mathrm{Hg} ; V=? ; n=0.210 \mathrm{~mol}$ $T=27^{\circ} \mathrm{C}$ b. $P=? \mathrm{~mm} \mathrm{Hg} ; V=644 \mathrm{~mL}$;

$$n=0.0921 \mathrm{~mol} ; T=303 \mathrm{~K}$$

c. $P=745 \mathrm{~mm} \mathrm{Hg} ; V=11.2 \mathrm{~L}$;

$$n=0.401 \mathrm{~mol} ; T=? \mathrm{~K}$$

What volume does $4.24 \mathrm{~g}$ of nitrogen gas occupy at $58.2^{\circ} \mathrm{C}$ and $2.04 \mathrm{~atm}$ ?

Given each of the following sets of values for an ideal gas, calculate the unknown quantity.

a. $P=1.01 \mathrm{~atm} ; V=$ ? $; n=0.00831 \mathrm{~mol} ; T=25^{\circ} \mathrm{C}$
b. $P=$ ? atm; $V=602 \mathrm{~mL} ; n=8.01 \times 10^{-3} \mathrm{~mol}$; $T=310 . \mathrm{K}$
c. $P=0.998 \mathrm{~atm} ; V=629 \mathrm{~mL} ; n=$ ? mol; $T=35^{\circ} \mathrm{C}$