The higher the critical temperature of the gas

Options

A. greater is its adsorption
B. lower its adsorption
C. lesser is the case of liquification
D. lesser is its volatile nature

Explanation

To solve the question regarding the relationship between the critical temperature of a gas and its properties, we can follow these steps:

### Step 1: Understand Critical Temperature
- **Definition**: The critical temperature (Tc) of a substance is the temperature above which its vapor cannot be liquefied, regardless of the pressure applied. This means that at temperatures above Tc, the substance exists only in the gaseous state.

### Step 2: Relationship Between Critical Temperature and Liquefaction
- **Liquefaction**: A higher critical temperature indicates that the gas can be liquefied more easily. This is because at higher temperatures, the kinetic energy of the molecules is greater, and they require more energy (in the form of pressure) to overcome intermolecular forces and remain in the gaseous state.

### Step 3: Van der Waals Forces
- **Intermolecular Forces**: The ease of liquefaction is directly related to the strength of intermolecular forces, specifically Van der Waals forces. A higher critical temperature suggests stronger Van der Waals forces, which facilitate the process of liquefaction.

### Step 4: Adsorption
- **Adsorption**: With stronger intermolecular forces (greater Van der Waals forces), the tendency for a gas to adsorb onto a surface also increases. Therefore, a gas with a higher critical temperature will exhibit greater adsorption.

### Step 5: Analyze the Options
- Given the options:
1. Greater is its adsorption.
2. Lower its adsorption.
3. Lesser is the case of liquefaction.
4. Lesser is its volatile nature.

- **Correct Option**: The first option is correct because a higher critical temperature correlates with greater adsorption due to stronger intermolecular forces.

### Final Answer
The correct statement is: "Greater is its adsorption."

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