The value of vander waal's constant a and b for two gases X and Y are 4.6,0.04 (for X) and 5.1, 0.06 (for Y). Which can be liquified easily an appolication of pressure :-

Options

A. X
B. Y
C. Both 1 & 2
D. None of these

Answer

To determine which gas, X or Y, can be liquefied more easily upon the application of pressure, we will analyze the given Van der Waals constants \(a\) and \(b\) for both gases.

### Step-by-Step Solution:

1. **Identify the Given Values:**
- For gas X: \(a_X = 4.6\), \(b_X = 0.04\)
- For gas Y: \(a_Y = 5.1\), \(b_Y = 0.06\)

2. **Calculate the Ratio \( \frac{a}{b} \) for Both Gases:**
- For gas X:
\[ \frac{a_X}{b_X} = \frac{4.6}{0.04} = 115 \]
- For gas Y:
\[ \frac{a_Y}{b_Y} = \frac{5.1}{0.06} = 85 \]

3. **Understand the Relationship with Critical Temperature:**
- The critical temperature \(T_c\) is related to the ratio \( \frac{a}{b} \) as follows:
\[ T_c \propto \frac{a}{b} \]
- This means that a higher \( \frac{a}{b} \) ratio indicates a higher critical temperature.

4. **Compare the Ratios:**
- Gas X has a ratio of \(115\) while gas Y has a ratio of \(85\).
- Since \(115 > 85\), it indicates that gas X has a higher critical temperature than gas Y.

5. **Conclusion:**
- A higher critical temperature means that gas X can be liquefied more easily upon the application of pressure compared to gas Y.

### Final Answer:
Gas X can be liquefied more easily upon the application of pressure.