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(B) For an ideal gas,the compressibility factor $Z = \frac{PV}{nRT} = 1$. For $n = 1$ mole,$Z = \frac{PV}{RT} = 1$.At low pressure,all real gases beha

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Curve $B$

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(B) For an ideal gas,the compressibility factor $Z = \frac{PV}{nRT} = 1$. For $n = 1$ mole,$Z = \frac{PV}{RT} = 1$.At low pressure,all real gases behave like an ideal gas,so $\frac{PV}{RT}$ approaches $1$ as $P$ approaches $0$.As pressure increases,the finite size of molecules and intermolecular forces cause deviations.For most real gases at high pressure,the volume of molecules becomes significant,making the gas less compressible than an ideal gas,which leads to $Z > 1$. This corresponds to an upward trend in the graph.Curve $B$ shows this characteristic behavior where the value of $\frac{PV}{RT}$ increases above $1$ as pressure increases.

An experiment is carried out on a fixed amount of gas at different temperatures and at high pressure such that it deviates from ideal gas behavior. The variation of $\frac{PV}{RT}$ with $P$ is shown in the diagram. The correct variation will correspond to

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