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

The enthalpy change for transition of liquid water to steam is 40.8 KJ mol^(1) at 737 K calculate DeltaS for the process

The enthalpy of vaporisation of water is 186.5 kJ mol^(-1) . The entropy of its vaporisation will be :

The enthalpy change for transition of liquid water to steam is 40.8 kJ mol^(-1) at 373K. Calculate Delta S for the process.

The enthalpy change for transition of liquid water to steam is 40.8 kJ mol^(-1) at 373K. Calculate Delta S for the process.

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 :