Calculate the entropy change when one mole of water at 373 K is converted into steam. Latent heat of vaporisation of water `(DeltaH_(v))` is `40.7 xx 10^(3) J mol^(-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 )

Calculate the entropy change when 1 gram of ice is converted to water. Given triangleH=6025 J/mole

What is meant by saying that the latent heat of vaporisation of water is 22.5 xx 10^(5) J//kg ?

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).

Caclulate the change in entropy of a 1000 kg of water converted into steam. Latent heat of steam =2.268xx10^(6)Jkg^(-1)

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))