$\frac{P}{3}$

$\frac{P}{5}$

$\frac{P}{7}$

$\frac{7P}{7+16}$

H₂

CO₂

C₂H₆

CClF₃

The average kinetic energy of the gas molecules is directly proportional to the temperature of the gas.

The volume of the gas molecules is negligible

The volume of the gas molecules is significant

The collision between gas molecules are elastic.

The attractive forces between gas molecules for ideal gas is negligible

Real gases will behave ideally at low temperature and high pressure

According to Charles' Law, at constant pressure, the volume of certain mass of gas is directly proportional to temperature

Molecules of ideal gas always collide with each other and the container walls, but there is no loss of kinetic energy.

0.20 atm

0.36 atm

0.25 atm

0.50 atm

Boyle 's Law states that the volume of the gas is directly proportional to its pressure

Kinetic theory of gases postulates that the volume of the gas particle is too small hence it can be ignored.

Larger value of a, in the van der Waals equation for a real gas, indicates a stronger attractive force between gas molecules.

1.9 L

2.1 L

3.4 L

4.3 L

0.30 atm

0.40 atm

0.90 atm

3.60 atm

low temperature and pressure

low temperature and elevated pressure

elevated temperature and low pressure

standard temperature and pressure