Gas Laws and Kinetic Theory

Gen Chem 1: Lecture 8

What causes atmospheric pressure?

The weight of the column of air molecules in the atmosphere above an object.

What is the SI unit of pressure?

Pascal (Pa), where 1 Pa = 1 N/m².

What is Amontons's Law?

The pressure of a given amount of gas is directly proportional to its temperature on the Kelvin scale when the volume is constant.

What does Charles's Law state?

The volume of a fixed amount of gas at constant pressure is directly proportional to its absolute temperature.

What is Boyle's Law?

The volume of a fixed quantity of gas at constant temperature is inversely proportional to the pressure.

What is Avogadro’s Law?

The volume of a gas at constant temperature and pressure is directly proportional to the number of moles of the gas.

What is the Ideal Gas Law?

PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.

How do you calculate density from the ideal gas equation?

d = MP/RT; where d is density, M is molar mass, P is pressure, R is the gas constant, and T is temperature.

What is Dalton's Law of Partial Pressures?

The total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the component gases.

What is the mean free path?

The average distance a molecule travels between collisions, which increases with decreasing pressure.

What is the definition of diffusion?

The process by which molecules disperse in space in response to differences in concentration.

What does the Kinetic-Molecular Theory assume about gas particles?

Gas particles are in constant motion, have elastic collisions, and do not experience attractive forces with each other.

What happens to the average speed of gas particles as pressure increases?

The average speed of gas particles increases due to the increased frequency and force of collisions.

What does compressibility factor (Z) represent?

The ratio of the actual volume of gas to the molar volume of an ideal gas at the same temperature and pressure.

Why do real gases deviate from ideal gas behavior?

Due to the volume of gas particles and attractive forces between them, especially at high pressures and low temperatures.