Chemistry - Thermodynamics - 1 Question with Solution | TestHub

For water${\mathrm{\Delta }}_{\mathrm{vap} }\mathrm{H}=41 \mathrm{kJ}{ \mathrm{mol}}^{-1}$at$373 \mathrm{K}$and 1 bar pressure. Assuming that water vapour is an ideal gas that occupies a much larger volume than liquid water, the internal energy change during evaporation of water is$\left({\mathrm{kJmol}}^{-1}\right)$:
[ Use$\left.:\mathrm{R}=8.3 \mathrm{J}{ \mathrm{mol}}^{-1}{ \mathrm{K}}^{-1}\right]$