Assertion. Greater the value of Henry's constant of a gas in a particular solvent, greater is the solubility of the gas at the same pressure and temperature.
Reason. Solubility of a gas is directly propportional to its Henry's constant at the same pressure and temperature.

Options

A. If both assertion and reason are true, and reason is the true explanation of the assertion.
B. If both assertion and reason are true, but reason is not the true explanation of the assertion.
C. If assertion is true, but reason is false.
D. If both assertion and reason are false.

Explanation

To solve the question, we need to analyze both the assertion and the reason provided in the context of Henry's law and the relationship between Henry's constant and the solubility of gases.

### Step-by-Step Solution:

**Step 1: Understanding Henry's Law**
- Henry's law states that at a constant temperature, the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of that gas above the liquid.
- Mathematically, it can be expressed as:
\[ C = k_H \cdot P \]
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