Question

Which one of the following statements regarding Henry’s law is not correct?

• A. Different gases have different $K_H$ (Henry’s law constant) values at the same temperature
• B. Higher the value of $K_H$ at a given pressure, higher is the solubility of the gas in the liquids
• C. The value of $K_H$ increases with increase of temperature and $K_H$ is function of the nature of the gas
• D. The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution

Answer 1

The correct option is B Higher the value of $K_H$ at a given pressure, higher is the solubility of the gas in the liquids

At constant temperature, solubility of a gas $\left(S\right)$ varies in versely with Henry’s law constant $\left(K_H\right)$.
$K_H=\frac{\text{Pressure}}{\text{Solubility of gas in a liquid}}=\frac{P}{S}$.
Thus, higher the value of $K_H$ at a given pressure, the lower is the solubility of the gas in the liquid.