If `Delta H_("vap")` of pure water at `100^(@)C` is `40.627 kJ mol^(-1)`. The value of `Delta S_("vap")` is

Standard enthaply of vaporisation Delta_(vap)H^(theta) for water at 100^(@)C is 40.66 kJ mol^(-1) . The internal energy of vapourisation of water at 100^(@)C (in kJ mol^(-1) ) is :

Standard enthalpy of vapourisation Delta_("vap")H^(-) for water at 100^@C is 40.66 kJ mol^(-1) . The internal energy of vapourisation of water at 100^@C (in kJ mol^(-1) ) is (Assume water vapour to behave like an ideal gas).

The enthalpy of vaporisation of water at 100^(@)C is 40.63 KJ mol^(-1) . The value Delta E for the process would be :-

The enthalpy of vaporisation of water at 100^(@)C is 40.63 KJ mol^(-1) . The value Delta E for the process would be :-

Delta H (vap) for water is 40.7 kJ mol^(-1) . The entropy of vaporisation of water is :