One mole of an ideal diatomic gas ( , ) is initially at pressure and temperature

PHYSICS · Multi-part · CBSE · Physics · Thermodynamics · Thermodynamics

Problem

One mole of an ideal diatomic gas (γ=1.4\gamma = 1.4, R=8.314 J mol−1 K−1R = 8.314\,\text{J\,mol}^{-1}\,\text{K}^{-1}) is initially at pressure 2.00×105 Pa2.00 \times 10^5\,\text{Pa} and temperature 300 K300\,\text{K}. The gas undergoes the following two-step reversible process: Step-1: Isothermal expansion at 300 K300\,\text{K} until its volume doubles. Step-2: Adiabatic compression until its pressure again becomes 2.00×105 Pa2.00 \times 10^5\,\text{Pa}. (i) Calculate the initial volume of the gas. (ii) Determine the work done by the gas during Step-1. (iii) Find the final volume after Step-2. (iv) Calculate the work done by the gas during Step-2. (v) Compute the net work done by the gas for the complete two-step path.

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