Two moles of an ideal mono-atomic gas ( , ) are initially at pressure and temperature…

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

Problem

Two moles of an ideal mono-atomic gas (

\gamma = \frac{5}{3}

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

) are initially at pressure

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

and temperature

400\,\text{K}

(state A). The gas is taken through the following reversible path: Step-1 (

A \rightarrow B

): Isothermal compression at

400\,\text{K}

from volume

6.00\,\text{L}

3.00\,\text{L}

. Step-2 (

B \rightarrow C

): Adiabatic expansion until the volume again becomes

6.00\,\text{L}

. (i) Calculate the work done by the gas and the heat exchanged during Step-1. (ii) Determine the pressure and temperature at state C. (iii) Calculate the work done by the gas during Step-2. (iv) Using your results, find the heat exchanged in Step-2 and hence the net heat exchanged over the whole path

A \rightarrow B \rightarrow C

Related theory

Browse the problem library