STATEMENT-1 : Plot of P vs 1/V (volume) is a straight line for an ideal gas.
STATEMENT-2 : Pressure is directly proportional to volume for an ideal gas.

Options

A. If both the statement are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1
B. If both the statement are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To analyze the statements provided, let's break down the concepts step by step.

### Step 1: Understand the Ideal Gas Law
The Ideal Gas Law is given by the equation:
\[ PV = nRT \]
where:
- \( P \) = pressure of the gas
- \( V \) = volume of the gas
- \( n \) = number of moles of the gas
- \( R \) = universal gas constant
- \( T \) = temperature in Kelvin

### Step 2: Analyze Statement 1
**Statement 1:** "Plot of P vs 1/V (volume) is a straight line for an ideal gas."

When we rearrange the Ideal Gas Law for a constant temperature, we can express pressure \( P \) in terms of \( V \):
\[ P = \frac{nRT}{V} \]
This shows that pressure \( P \) is inversely proportional to volume \( V \).

If we plot \( P \) against \( \frac{1}{V} \), we can rewrite the equation as:
\[ P = nRT \cdot \frac{1}{V} \]
This is in the form of \( y = mx \), where:
- \( y \) is \( P \)
- \( x \) is \( \frac{1}{V} \)
- \( m \) (the slope) is \( nRT \)

Thus, the plot of \( P \) versus \( \frac{1}{V} \) is indeed a straight line. Therefore, **Statement 1 is correct.**

### Step 3: Analyze Statement 2
**Statement 2:** "Pressure is directly proportional to volume for an ideal gas."

From the Ideal Gas Law, we see that:
\[ P \propto \frac{1}{V} \]
This indicates that pressure is inversely proportional to volume, not directly proportional. Therefore, as the volume increases, the pressure decreases, and vice versa. Thus, **Statement 2 is false.**

### Conclusion
- **Statement 1 is correct.**
- **Statement 2 is false.**

### Final Answer
- **Statement 1:** True
- **Statement 2:** False

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