Physics

Problem

One mole of an ideal diatomic gas (

\gamma = 1.4

R = 8.314\,\text{J\,mol}^{-1}\,\text{K}^{-1}

) is initially at pressure

2.00 \times 10^5\,\text{Pa}

and temperature

300\,\text{K}

. The gas undergoes the following two-step reversible process: Step-1: Isothermal expansion at

300\,\text{K}

until its volume doubles. Step-2: Adiabatic compression until its pressure again becomes

2.00 \times 10^5\,\text{Pa}

. a. (i) Calculate the initial volume of the gas. b. (ii) Determine the work done by the gas during Step-1. c. (iii) Find the final volume after Step-2. d. (iv) Calculate the work done by the gas during Step-2. e. (v) Compute the net work done by the gas for the complete two-step path.

Browse the problem library