Chapter 8: The Gas Phase (9%)

fluids, compressible

gases are ______ and therefore conform to the shapes of their containers and they are also easily _____________

temperature, pressure, volume, number of moles (T, P, V, n)

the 4 variables that describe gas systems

increases, decreases

A simple mercury barometer measures incident (usually atmospheric) pressure. As pressure ___________, more mercury is forced into the column, increasing its height. As pressure ____________, mercury flows out of the column under its own weight, decreasing its height.

237K, 1atm

state the temperature and pressure defined as standard temperature and pressure (STP)

have no intermolecular forces, occupy no volume

the 2 characteristics of an ideal gas

pressure x volume = number of moles x ideal gas constant x temperature

(PV = nRT)

write out the formula for the ideal gas law

density = mass / volume = (pressure x molar mass) / (ideal gas constant x temperature)

write out the formula for calculating the density of a gas (derived from the ideal gas law PV = nRT)

P1V1/T1 = P2V2/T2

write out the formula for the combined gas law (derived from the ideal gas law PV = nRT)

V2 = V1 (P1/P2) (T2/T1)

write out the formula for calculating the change in volume (derived from the combined gas law P₁V₁/T₁ = P₂V₂/T₂)

volume

Regardless of the identity of the gas, equimolar amounts of two gases will occupy the same _________ at the same temperature and pressure

22.4 L

the volume that one mole of an ideal gas occupies at STP

pressure, temperature, direct

Avogadro’s principle is a special case of the ideal gas law for which the __________ and ______________ are held constant; it shows a _________ relationship between number of moles of gas and volume

n1/V1 = n2/V2

write out the formula for Avogadro’s principle in which pressure and temperature remain constant

temperature, number of moles, inverse

Boyle’s law is a special case of the ideal gas law for which the _____________ and ________ ___ ______ are held constant; it shows an _________ relationship between pressure and volume

P1V1 = P2V2

write out the formula for Boyle’s law in which temperature and number of moles remain constant

pressure, number of moles, direct

Charles’s law is a special case of the ideal gas law for which the __________ and ________ ___ ______ are held constant; it shows a _________ relationship between temperature and volume

V1/T1 = V2/T2

write out the formula for Charles’s law in which pressure and number of moles are constant

volume, number of moles, direct

Gay-Lussac’s law is a special case of the ideal gas law for which the _________ and ________ ___ ______ are held constant; it shows a _________ relationship between temperature and pressure

P1/T1 = P2/T2

write out the formula for Gay-Lussac’s law in which volume and number of moles remain constant

inverse, direct

the combined gas law shows an _________ relationship between pressure and volume along with _________ relationships between pressure and volume with pressure

individual, pressures, mole fractions, pressure, partial pressures

Dalton’s law of partial pressures states that ____________ gas components of a mixture of gases will exert individual __________ in proportion to their ______ _________. The total _________ of a mixture of gases is equal to the sum of the ________ _________ of the component gases.

(moles of individual gas / total moles of gas) x total pressure

write out the formula for calculating the partial pressure of a gas according to Dalton’s law of partial pressures

dissolved, partial pressure, vapor pressure

Henry’s law states that the amount of gas ___________ in solution is directly proportional to the _________ __________ of that gas at the surface of the solution (aka its ________ __________)

vapor pressure

the pressure exerted by evaporated particles above the surface of a liquid

increase

The solubility of a gas will __________ with increasing partial pressure of the gas

volume, intermolecular, random collisions, elastic, temperature

According to the kinetic molecular theory, which attempts to explain the behavior of gas particles, gas particles have negligible __________, they do not experience _____________ forces, they undergo __________ ___________ with each other and the walls of the container, collisions are ________, and the average kinetic energy of the gas particles is directly proportional to ______________

faster, slower

According to the kinetic molecular theory, the higher the temperature, the _________ the molecules move. The larger the molecules, the _________ they move.

faster

Graham’s law states that gases with lower molar masses will diffuse or effuse ________ than gases with higher molar masses at the same temperature

square root (molar mass of gas 2 / molar mass of gas 1)

write out the formula for Graham’s law which calculates the rates of diffusion for two gasses (diffusion rate of gas 1/ diffusion rate of gas 2 = ?)

diffusion

the spreading out of particles from high to low concentration

effusion

the movement of gas from one compartment to another through a small opening under pressure

slower, slower

heavier gasses dissolve _________ than lighter ones because particles with greater mass travel at a _________ average speed

low temperature, high pressure (aka low volume)

the 2 conditions under which real gases start to deviate from ideal behavior

less, intermolecular attractions

at moderately high pressures, low volumes, or low temperatures, real gases will occupy _____ volume than predicted by the ideal gas law because the particles have _____________ ___________

more, take up space

at extremely high pressures, low volumes, or low temperatures, real gases will occupy _____ volume than predicted by the ideal gas law because the particles ______ ___ _______