Question

Calculate the work done during isothermal reversible expansion of one mole ideal gas from 10 atm to 1 atm at 300 K.

Answer 1

work done =$-2.303nRTlog\left(\frac{P_1}{P_2}\right)$

$=-2.303\times 8.314\times 300log\left(\frac{1}{10}\right)$

$=-2.303\times 8.314\times 300$

$=-5.74kJ$

$\therefore$ work done will be 5.74 kJ.