Question

Which one of the following is the correct PV vs P plot at constant temperature for an ideal gas ? (P and V stand for pressure and volume of the gas respectively) 

• A. A
• B. B
• C. C
• D. D

Hint:

For an ideal gas, any plot of \( PV \) against \( P \) or \( V \) at constant temperature will always be a horizontal straight line. Deviations from this line indicate non-ideal (real) gas behavior.

Answer 1

The Correct Option is D

To solve this question, we need to understand the behavior of an ideal gas at constant temperature (isothermal conditions) as described by the Ideal Gas Law.

The Ideal Gas Law is given by:

PV = nRT

Where:

• P is the pressure of the gas.
• V is the volume of the gas.
• n is the number of moles of the gas (constant).
• R is the universal gas constant (constant).
• T is the temperature (constant in this case).

At constant temperature, the product PV is a constant, hence PV = \text{constant}.

Therefore, if temperature is constant, the plot of PV against P should be a straight line parallel to the x-axis (pressure axis), indicating that PV does not depend on P.

From the given options, Option D correctly represents this behavior as a horizontal line. Here is the diagram for reference:

Therefore, the correct answer is Option D.