State Henry's law. What is the effect of temperature on the solubility of a gas in a liquid ?

Explanation

Henry's Law states that the solubillity of a gas in a liquid is directly proportional to the
pressure of the gas. If we use the mole fraction of a gas in the solution as a measure of its
solubility ,then it can be said that the mole fraction of gas in the solution is proportional to
the partial pressure of the gas over the solution. The most commonly used form of Henry's
Law states that ''the partial pressure of a gas in vapour phase (p) is directly proportional to
the mole fraction of the gas (x) in the solution,i.e
`p propto x`
`p =K_(H)x`
The solubility of gases is dependent on temperature. An increase in temperature results in a
decrease in gas solubility in liquid, while a decrease in temperature results in an increase of
gas solubility in liquid .
As increase in temperature causes an increase in kinetic energy, resulting in a more rapid
motion of molecules, breaking intermolecular bonds which enable molecular to escape from
the solution allowing the gases dissolved to evaporate more readily. Hence causing decrease in the solubility of gases in liquids.