State Henry’s law. Why do gases always tend to be less soluble when the temperature is raised?

OR

State Raoult’s law for the solution containing volatile compounds. Write two differences between an ideal and a non-ideal solution.

Henry’s law states that the solubility of a gas in a liquid is directly proportional to its pressure over the liquid. As we increase the temperature the particles of gas come in better proximity with the molecules of liquid and hence the temperature increases. He measures the solubility of the gas in terms of its mole fraction. The gases always tend to be less soluble in liquid when temperature is raised because on high temperature the particles of gases move away from each other and hence escapes from liquid. So they tend to be less soluble on high temperature.

OR

Raoult’s law states that a solution containing two volatile components, the vapour pressure of any component of the solution is directly proportional to its mole fraction in liquid phase.