One mole of an ideal gas at pressure P 0 and temperature T 0 with volume V 0 is expanded isothermally to twice its volume. It is then compressed at constant pressure to V 0 /2 , and the gas is

Question

One mole of an ideal gas at pressure P 0 ​ and temperature T 0 ​ with volume V 0 ​ is expanded isothermally to twice its volume. It is then compressed at constant pressure to V 0 ​ /2 , and the gas is brought to its original state by a process in which P ∝ V (Pressure is directly proportional to volume). The correct representation of this process is:

TestHub · Accepted Answer

The process involves three steps:

1. Isothermal expansion: $P_{0} V_{0} = P_{1} (2 V_{0}) \Rightarrow P_{1} = P_{0} /2$ .

2. Isobaric compression: Pressure remains $P_{1} = P_{0} /2$ . Volume changes from $2 V_{0}$ to $V_{0} /2$ .

3. $P \propto V$ : This is a straight line through the origin on a P-V diagram. The gas returns to $(P_{0}, V_{0})$ .

Plotting these steps on a P-V diagram matches option C.

Physics - Heat & Thermo Question with Solution | TestHub

Options:

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