Learning Objectives
Chapter 13
Vocabulary: kinetic energy kinetic theory gas pressure vacuum
atmospheric pressure barometer vaporization evaporation
sublimation deposition melting freezing
normal boiling point melting point triple point elastic collision
endothermic exothermic
Describe the assumptions of the kinetic theory as it applies to gases.
Understand the effects collisions have on gas pressure.
Define the relationship between Kelvin temperature and average kinetic energy.
Use a phase diagram to
identify the conditions necessary for each phase change,
identify the phases present under various temperature and pressure conditions,
describe how phases change when pressure and temperature conditions change,
identify the conditions in which triple point exists.
Learning Objectives
Chapter 14
Vocabulary: compressibility temperature ideal gas real gas
effusion diffusion partial pressure
Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses.
Explain why gases are easier to compress than solids or liquids are.
Explain how the temperature, volume, pressure, and amount affect gas behavior.
Use Boyle’s law, Charles’ Law, and Gay-Lussac’s Law, combined gas law, and ideal gas law to solve problems involving gases.
Compare and contrast real and ideal gases.
Relate the total pressure of a mixture of gases to the partial pressures of the component gases. (Dalton’s Law of Partial Pressures)
Use stoichiometry to solve molar volume problems. (Gas Stoichiometry)