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

Options

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

Explanation

To determine which statement regarding Henry's law is not correct, we first need to understand the fundamentals of Henry's law. Here’s a step-by-step breakdown of the solution:

### Step 1: Understand Henry's Law
Henry's law states that the amount of gas dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid. Mathematically, it can be expressed as:
\[ P = k_H \cdot C \]
where:
- \( P \) = partial pressure of the gas,
- \( k_H \) = Henry's law constant (proportionality constant),
...