Assuming that water vapour is an ideal gas, the internal energy change $\left( {\Delta U} \right)$ when $1$ mol of water is vapourised at $1$ bar pressure and ${100^ \circ }C$ (Given : molar enthalpy of vapourisation of water at $1$ bar and $373$ $K$ $ = 41\,kJ\,mo{l^{ - 1}}\,$ and $R = 8.3\,J\,mo{l^{ - 1}}\,{K^{ - 1}}$ )

Question

Assuming that water vapour is an ideal gas, the internal energy change $\left( {\Delta U} \right)$ when $1$ mol of water is vapourised at $1$ bar pressure and ${100^ \circ }C$ (Given : molar enthalpy of vapourisation of water at $1$ bar and $373$ $K$ $ = 41\,kJ\,mo{l^{ - 1}}\,$
and $R = 8.3\,J\,mo{l^{ - 1}}\,{K^{ - 1}}$ )

$41.00\,kJ\,mo{l^{ - 1}}$

$4.100\,kJ\,mo{l^{ - 1}}$

$3.7904\,kJ\,mo{l^{ - 1}}$

$37.904\,kJ\,mo{l^{ - 1}}$

Solution

Please login to view the detailed solution steps...

Go to DASH