The change of state from liquid H₂O to gaseous H₂O has ∆H = +9.72 kcal/mol(+40.7 kJ/mol) and ∆S = -26.1 cal/(mol • K) [-109 J/(mol •K)].

a. Is the change from liquid to gaseous H2O favored or unfavored by ∆H? By ∆S?

The change of state from liquid H₂O to gaseous H₂O has ∆H = +9.72 kcal/mol(+40.7 kJ/mol) and ∆S = -26.1 cal/(mol • K) [-109 J/(mol •K)].

b. What are the values of ∆H and ∆S (in kcal/mol and kJ/mol) for the change from gaseous to liquid H2O?

Would you expect the boiling points to increase or decrease in the following series? Explain.

a. Kr, Ar, Ne

A local weather station reports the barometric pressure as 29.5 inHg (inches of Hg). Convert this pressure to torr and to atm.

Determine the percent composition of air in the lungs from the following composition in partial pressures: PN₂= 573 mmHg, PO₂ = 100 mmHg, PCO₂ = 40 mmHg, and PH₂O = 47 mmHg; all at 37 °C and 1 atm pressure.

Compare the ∆H_vap values for water, isopropyl alcohol, ether, and ammonia, and order them from lowest to highest. Explain the rank order based on intermolecular attractive forces.

Assume that you have a sample of gas at 350 K in a sealed container, as represented in part (a). Which of the drawings (b)–(d) represents the gas after the temperature is lowered from 350 K to 150 K and if the gas has a boiling point of 200 K? Which drawing represents the gas at 150 K if the gas has a boiling point of 100 K?

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List four common units for measuring pressure.

Which assumptions of the kinetic–molecular theory explain the behavior of gases described by Boyle's law? Explain your answer.

Which assumptions of the kinetic–molecular theory explain the behavior of gases described by Charles's law? Explain your answer.

Which assumptions of the kinetic–molecular theory explain the behavior of gases described by Gay-Lussac's law? Explain your answer.

A gas has a volume of 2.84 L at 1.00 atm and 0 °C. At what temperature does it have a volume of 7.50 L at 520 mmHg?

Explain Avogadro's law using the kinetic–molecular theory of gases.

How many molecules are in 1.0 L of O₂ at STP? How may grams of O₂?

What is the mass of CH₄ in a sample that occupies a volume of 16.5 L at STP?

How does the ideal gas law differ from the combined gas law?

Which sample contains more molecules: 2.0 L of Cl₂ at STP or 3.0 L of CH₄ at 300 K and 1150 mmHg? Which sample weighs more?

What is meant by partial pressure?

What is a liquid's heat of vaporization?

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

List three kinds of crystalline solids, and give an example of each.

Use the kinetic–molecular theory to explain why gas pressure increases if the temperature is raised and the volume is kept constant.

Obtain phase diagrams for water and carbon dioxide.

a. Based on the phase diagram for water, explain how it is possible to skate on ice, that is, solid water.

Obtain phase diagrams for water and carbon dioxide.

b. Would it be possible to skate on 'dry ice,' that is, solid CO₂?