[" The enthalpy of vapourisation of water at "100^(@)C" is "],[40.63kymol" .The value of "/_f" for this process would "],[" be "(k" JImol) "]

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 :-

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

Standard enthalpy of vaporisation DeltaV_(vap).H^(Theta) for water at 100^(@)C is 40.66kJmol^(-1) .The internal energy of Vaporization of water at 100^(@)C("in kJ mol"^(-1)) is

Standard enthalpy of vapourisation Delta_(vap) H^- for water at 100° C is 50.66 kJmol^(–1) . The internal energy of vapourisation of water at 100°C (in kJmol^(–1) ) is ?

Standard enthalpy of vapourisation Delta_(vap) H^- for water at 100° C is 44.66 kJmol^(–1) . The internal energy of vapourisation of water at 100°C (in kJmol^(–1) ) is ?