The Ideal Gas Law (copy)

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atomic mass unit symbol

Avogadro’s number

The number of atoms per mole

Mole

the SI base unit for expressing “the amount of a substance”

Ideal Gas Law

expresses the relationship between the absolute pressure, the Kelvin temperature, the volume, and the number of moles of the gas

Inversely proportional

At constant temperature, the pressure is (?) to the volume

Proportional

At constant volume, the pressure is (?) to the temperature

Proportional

The pressure is (?) to the amount of gas

R = 8.31 J/(mol K)

universal gas constant

Boltzmann’s constant

he constant k is referred to as (?), in honor of the

Austrian physicist Ludwig Boltzmann

Boyle’s Law

• for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure

• P1V1 = P2V2

Charle’s Law

states that the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant

Kinetic Theory of Gases

• The particles are in constant, random motion, colliding with each other and with the walls of the container.

• Each collision changes the particle’s speed.

• As a result, the atoms and molecules have different speeds.

directly proportional

The Kelvin temperature is (?) to the average kinetic energy per particle in an ideal gas, no matter what the pressure and volume are

Diffusion

The process in which molecules move from a region of higher concentration to one of lower concentration

Fick’s Law of Diffusion

The mass m of solute that diffuses in a time t through a solvent contained in a channel of length L and cross sectional area A is

m = (𝑫𝑨𝜟𝑪) 𝒕 / 𝑳