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The value of C_{P} – C_{V} is 1.00 R for a gas sample in state A and is 1.08R in state B. Let P_{A}, P_{B} denote the pressures and T_{A,} and T_{B} denote the temperatures of the states A and B respectively. Most likely

For gas in state A, C_{p} - C_{v} = R. This represents an ideal gas. Now, for an ideal gas, we require very high temperature and very low pressure compared to a real gas

For gas in state B, C_{p} - C_{v} = 1.08R, which represents a real gas. Since gas A was ideal, its pressure must be much lower than that of B and temperature must be much higher than that of A.

Hence, we require the condition p_{A} < p_{B} and T_{A} > T_{B}. This is given by option (a).

Options (b), (c) and (d) are incorrect because none of those satisfies the conditions for an ideal gas.

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