Explanation:
Ideal gas law states that the product of the pressure and the volume of one gram molecule of an ideal gas is equal to the product of the absolute temperature of the gas and the universal gas constant.
Mathematically, PV = nRT
where, P = pressure
V = volume
n = number of moles
R = gas constant
T = absolute temperature
A gas behaves ideally at high temperature and low pressure because when pressure is low and temperature is high then there will be more number of collisions between the gas particles. As a result, kinetic energy of molecules will increase hence, molecule's size will become less significant as compared to the empty space between them.
Therefore, conditions for which the ideal gas law will be most accurate are as follows.
- high temperatures
- low pressures
