Question

According to Henry’s law, the solubility of a gas in a given volume of liquid increases with increase in:
A.Temperature
B.Pressure
C.Both A and B
D.None of the above

Answer 1

To answer this question, you must recall the Henry’ law of solubility. Henry's law gives a relation of the solubility of gas using partial pressure above the solution and the mole fraction of the gas in the solution.
Formula used: ${{P}} = {{{K}}_{{H}}}{{\chi }}$
Where, $P$ denotes the partial pressure of the gas above the surface of solution
${K_H}$ denotes the Henry’s law constant
And, $\chi$ denotes the mole fraction of the gas in the solution

Complete answer:
Henry’s law is a gas solubility law which proposes that the amount of gas which is dissolved in a given liquid is directly proportional to the partial pressure of that gas present above the liquid at constant temperature conditions. The proportionality constant ${K_H}$is known as the Henry’s Law constant and it has different values for different gases at constant temperature.
Hence we can say that on increasing the pressure of the gas, the mole fraction of the gas in the solution increases. So B is the correct answer.
The Henry’s law constant is directly proportional to the temperature. From the equation of the Henry’s Law constant, ${{P}} = {{{K}}_{{H}}}{{\chi }}$ we can see that the mole fraction of the gas is inversely proportional to the Henry’s Constant. Hence we can say that the henry’s law constant is inversely proportional to the solubility of the gas in solution.
Thus, the solubility of a gas decreases with increase in temperature.

Thus, the correct answer is B.
Note:
Apart from the temperature and pressure, the solubility of gas also depends on the nature of gas, nature of the solvent and the interactions between them.