Question

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

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

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.

Different gases have different $K_H$ values at the same temperature. This suggests that $K_H$ is a function of the nature of the gas.
$\therefore$ Statement (A) and (D) both are correct.

The most commonly used form of Henry’s law states that “the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution” and is expressed as:

$p=K_{H}X$

Here $K_H$ is Henry’s law constant.

$\therefore$ Statement (C) is correct.

Thus, $K_H$ is directly proportional to the pressure.

More is $K_H$ less is solubility, lesser solubility is at higher temperature.

So, more is the temperature, more is the $K_H$.

The only incorrect option is B.