Question

Calculate the work done in joules when $3$ moles of an ideal gas at ${27}^{o}C$ expands isothermally and reversibly from $10$ atm to $1$ atm.
$(1atm=1.013\times {10}^{5}N{m}^{-2})$.

Answer 1

For an isothermal process

$W=2.303nRTlog\frac{P_1}{P_2}$ where$P_1=10$ $atm$ $P_2=1$ $atm$

$W=2.303\times 3\times 8.314\times 300\times log\frac{10}{1}$

$W=17232.42$ $J$

$W=\mathrm{17.232.42}$ $KJ$