Three moles of an ideal diatomic gas undergoes a change in state from A to B reversibly as follows : Which of the following statements is/are correct regarding the above process :

Engineering

Chemistry

First Law and Various Process

Ideal Gas Equation

Gibbs Free Energy Entropy and Spontaneity

Question

Three moles of an ideal diatomic gas undergoes a change in state from A to B reversibly as follows : Which of the following statements is/are correct regarding the above process :

Work done on the gas is 2700 R.

In the above process, pressure varies inversely with square of volume.

Heat supplied to the gas is 4050 R.

Data insufficient for the calculation of work and heat supplied.

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From graph, slope = –1

∴ eq = log₁₀V + log₁₀T = constant

∴ VT = constant or PV² = constant

$C = C_{v} + \frac{R}{1 - n} ∴ C = \frac{5 R}{2} + \frac{R}{1 - 2} = \frac{3 R}{2}$

$∴ q = nCΔT = 3 \times \frac{3 R}{2} \times (1000 - 100) = 4050 R$

$ΔU = nCvΔT = 3 \times \frac{5 R}{2} \times (1000 - 100) = 6750 R$

∴ W = ΔU – q = 6750 R – 4050 R = 2700 R