Value of Henry's constant `K_(H)`…

Options

A. greater for gases with higher solubility
B. greater for gases with lower solubility
C. constant for all gases
D. not related to the solubility of gases

Explanation

To solve the question regarding the value of Henry's constant \( K_H \), we will follow these steps:

### Step 1: Understand Henry's Law
Henry's Law states that the partial pressure of a gas (\( P \)) above a liquid is directly proportional to the concentration (or solubility) of that gas in the liquid (\( X \)). This can be mathematically expressed as:
\[ P = K_H \times X \]
Where:
- \( P \) = partial pressure of the gas
- \( K_H \) = Henry's constant
- \( X \) = solubility of the gas in the liquid

### Step 2: Analyze the Relationship
From the equation \( P = K_H \times X \), we can rearrange it to express \( K_H \):
\[ K_H = \frac{P}{X} \]
This indicates that Henry's constant \( K_H \) is inversely proportional to the solubility \( X \).

### Step 3: Determine the Implications of Inversely Proportional Relationship
Since \( K_H \) is inversely proportional to \( X \):
- If the solubility \( X \) of a gas in a liquid decreases, \( K_H \) will increase.
- Conversely, if the solubility \( X \) increases, \( K_H \) will decrease.

### Step 4: Conclusion About Gases with Lower Solubility
From the above relationship, we can conclude that:
- Gases that have lower solubility in a liquid will have a higher value of Henry's constant \( K_H \).
- Therefore, the value of \( K_H \) is greater for gases with lower solubility.

### Final Answer
Thus, the correct conclusion is that the value of Henry's constant \( K_H \) is greater for gases with lower solubility.

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