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)`.

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

Find the entropy change for vaporisation of water to steam at 100^@C in JK^(-1)mol^(-1) if heat of vaporisation is 40.8 kJ mol^(-1) .

Calculate the entropy changes of fustion and vaporisation for chlorine from the following data: Delta_(fus)H = 6.40 kJ mol^(-1) , melting point =- 100^(@)C Delta_(vap)H = 20.4 kJ mol^(-1) , boiling point =- 30^(@)C

Calculate the entropy changes of fusion and vapourisation for chlorine from the following data: Delta_(fus)H = 6.40 kJ mol^(-1) , melting point =- 100^(@)C Delta_(vap)H = 20.4 kJ mol^(-1) , boiling point =- 30^(@)C

Calculate entropy changes of fusion and vaporisation for chlorine from the following data : Delta_(fus) H = 6.40 kJ "mol"^(-1) m.p = -102^(@)C Delta_(vap) H = 20.4 kJ mol^(-1) b.p = - 34^(@)C

If water vapour is assumed to be a perfect gas, molar enthalpy change for vaporization of 1 mol of water at 1 bar and 100^(@) C is 41 kJ mol^(-1) . Calculate the internal energy, when 1 mol of water is vapourised at one bar pressure and 100^(@) C.

If water vapour is assumed to be a perfect gas, molar enthalpy change for vaporization of 1 mol of water at 1 bar and 100^(@) C is 41 kJ mol^(-1) . Calculate the internal energy, when 1 mol of water is vapourised at one bar pressure and 100^(@) C.

If water vapour is assumed to be a perfect gas, molar enthalpy change for vaporization of 1 mol of water at 1 bar and 100^(@)C is 51 kJ mol ^(-1) . Calculate the internal energy, when 1 mol of water is vapourised at one bar pressure and 100^(@)C .