The van der Waals' constant 'a' for `CO_(2)` gas is greater than that of `H_(2)` gas. Its mean that the

Options

A. strength of van der Waals' force of `CO_(2)` gas is less than that of `H_(2)` gas
B. strength of van der Waals' force of `CO_(2)` gas is equal to that of `H_(2)` gas
C. `CO_(2)` gas can be more easily liquified
D. `H_(2)` gas can be more easily liquified

Explanation

To solve the question regarding the van der Waals' constant 'a' for CO₂ gas being greater than that of H₂ gas, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the van der Waals Equation**:
The van der Waals equation is an adjustment of the ideal gas law that accounts for intermolecular forces and the volume occupied by gas molecules. It is given by:
\[ \left(P + \frac{a(n/V)^2}{V - nb}\right)(V - nb) = nRT \]
Here, 'a' is the van der Waals constant related to the attractive forces between molecules.

2. **Interpret the Constant 'a'**:
The constant 'a' indicates the strength of the intermolecular attractions. A higher value of 'a' suggests stronger intermolecular forces. Therefore, if the value of 'a' for CO₂ is greater than that for H₂, it implies that CO₂ has stronger intermolecular attractions compared to H₂.

3. **Relate to Liquefaction**:
Stronger intermolecular forces mean that the gas can be more easily liquefied. This is because the attractive forces can pull the molecules closer together, allowing them to transition from a gaseous state to a liquid state more readily.

4. **Conclusion**:
Since the van der Waals constant 'a' for CO₂ is greater than that for H₂, it indicates that CO₂ can be more easily liquefied due to its stronger intermolecular interactions.

### Final Answer:
The greater value of the van der Waals constant 'a' for CO₂ gas compared to H₂ gas means that CO₂ gas can be more easily liquefied because it has stronger intermolecular interactions.

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