Entropy change involve in conversion of `1` mole of liquid water at `373K` to vapour at the same temperature (latent heat of vaporisation of water=`2.257kJg^(-1))`

Entropy change involve in conversation of 1 mole of liquid water at 373K to vapour at the same temperature (latent heat of vaporisation of water= 2.257kJg^(-1))

Calculate the entropy change involved in convertion of 1 mole of water at 373 K to vapours at the same temperature. Latent heat of vaporisation of water = 2.257 kJ g^(-1) .

Calculate the entropy change involved in the conversion of one mole of water at 373 K to vapour at the same temperature.(Latent heat of vaporisation of water at this temperature , Delta H_vap = 2.257 kJg^-1 )

Entropy change involved in the conversion of 1 mole of liquid water at 373 K to vapour at the same temperature will be ____ ( DeltaH_"vap"=2.257 kJ g^(-1) )

Calculate the entropy change involved in the vaporisation of water at 373 K to vapours at the same temperature(Latent heat of vaporisation = 2.275 kJ/g).