Question

A piston filled with 0.04 moles of an ideal gas expands reversibly from 50.0 L to 375.0 L at a constant temperature of ${37.0}^{\circ }C$. As it does so, it absorbs 208 J of heat energy. The value of work done (in $J$) for the process will be: (R = 8.314 J/mol K, ln 7.5 = 2.01)

Answer 1

The process is isothermal expansion, hence
q = - W
$\Delta E=0$
$W=-2.303nRTlog\frac{V_2}{V_1}$
$=-2.303\times 0.04\times 8.314\times 310\times log\frac{375}{50}$
$=-208J$
W = $-208.0J$ (expansion work)