91Ó°ÊÓ

If \(18.0 \mathrm{~g}\) of \(\mathrm{O}_{2}\) gas has a temperature of \(350 \mathrm{~K}\) and a pressure of \(550 \mathrm{mmHg}\), what is its volume?

How many moles of a gas will occupy a volume of \(0.55 \mathrm{~L}\) at a temperature of \(347 \mathrm{~K}\) and a pressure of \(2.5 \mathrm{~atm} ?\)

What is meant by partial pressure?

What is Dalton's law?

If the partial pressure of oxygen in air at 1.0 atm is \(160 \mathrm{mmHg},\) what is its partial pressure on the summit of Mt. Whitney, where atmospheric pressure is \(440 \mathrm{mmHg}\) ? Assume that the percent oxygen is the same.

Scuba divers who suffer from decompression sickness are treated in hyperbaric chambers using heliox ( \(21 \%\) oxygen, \(79 \%\) helium) at pressures up to 120 psi. Calculate the partial pressure of \(\mathrm{O}_{2}\) (in \(\mathrm{mmHg}\) ) in a hyperbaric chamber under these conditions.

What is a liquid's heat of vaporization?

What is the effect of pressure on a liquid's boiling point?

Which of the following substances would you expect to have the higher vapor pressure: \(\mathrm{CH}_{3} \mathrm{OH}\) or \(\mathrm{CH}_{3} \mathrm{Cl}\) ? Explain.

The heat of vaporization of water is \(40.7 \mathrm{~kJ} / \mathrm{mol}\). (a) How much heat (in kilojoules) is required to vaporize \(3.00 \mathrm{~mol}\) of \(\mathrm{H}_{2} \mathrm{O} ?\) (b) How much heat (in kilojoules) is released when \(320 \mathrm{~g}\) of steam condenses?