`Delta S` for vapouization of 900g water (in KJ/K ) is `Delta H_(Vap)=40KJ(mol)^-1 `

The enthalpy change for the transition of liquid water to steam, Delta_(vap) " H=37.3 kJ " mol^-1 at 373 K. The entropy change for the process is __________ .

Calculate the entropy change for vaporization of 1mol of liquid water to stem at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .

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

Calculate the standard enthalpy of solution of AgCl(s) in water DeltaH_(f)^(0)(AgCl,s)= -127.07kJ mol^(-1), Delta H_(f)^(0)(Ag^(+),aq)=105.58 kJ mol^(-1),DeltaH_(f)^(0)(Cl^(-),aq)= -167.35 kJ mol^(-1)

For a substance with the value of DeltaH_(vap) and DeltaS_(vap) given below, what is its normal boiling point in .^(@)C (DeltaH_(vap)=59.0 kJ mol^(-1), DeltaS_(vap)=93.65 Jmol^(-1))

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 737 K calculate DeltaS for the process