Gaseous State

Question 1

Avogadro’s Law

Answer 1

Volume, V, of a gas is directly proportional to the amount of gas particles (in mol) at constant temperature and pressure

V direct to n

Question 2

Boyle’s Law

Answer 2

Volume, V, of a fixed mass of gas is inversely proportional to its pressure, p, at a constant temp

V inverse to p

Question 3

Charles’ Law

Answer 3

Volume, V, of a fixed mass of gas is directly proportional to its absolute temperature, T, at a constant pressure

V direct to T

Question 4

Gay-Lussac’s Law

Answer 4

Pressure, p, of a fixed mass of gas is directly proportional to it’s absolute temperature, T, at a constant volume

p direct to T

Question 5

Assumptions of the kinetic theory

Answer 5

1. There are no intermolecular forces of attraction between the particles of an ideal gas
2. The volume of the ideal gas is negligible as compared to the volume of the container
3. Collisions between particles of an ideal gas are perfectly elastic i.e. no loss of KE upon collision
4. Gas particles are in rapid, continuous and random motion
5. The average KE of the particles is proportional to its absolute temperature measured in Kelvin

Question 6

Gas deviates more from ideal behaviour at.. (1)

Answer 6

High pressure because
- volume of container decreases and particles are packed closer together
- so the volume of the particles become significant compared to the volume of the container

Question 7

Gas deviates more from ideal behaviour at.. (2)

Answer 7

Lower temperature because
- The particles have less KE and will move slower, hence collide with one another with less force
- Makes the IMOF more significant compared to the forces of intermolecular collisions

Question 8

Dalton’s Law of partial pressure

Answer 8

The total pressure of a mixture of gases that do not react chemically with one another is the sum of the partial pressures of the constituent gases