The latent heat of vaporisation of water at `100 ^(@)C` is `540 cal g^(-1)`. Calculate the entropy increase when one mole of water at `100^(@)C` is evaporated

Latent heat of vaporisation of water is 540cal g^(-1) at 100^(@)C calculate the entropy change when 1000 g water is converted to steam at 100^(@)C

Latent heat of vaporisation of water is 540 cal/gm.Explain the meaning of the statement.

One moles of strem is compressed reversibly of water at boiling point 100^(@)C . The heat of vapourisation of water at 100^(@)C and 1atm is 540cal g^(-1) . Calculate DeltaU and DeltaH .

One moles of strem is compressed reversibly of water at boiling point 100^(@)C . The heat of vapourisation of water at 100^(@)C and 1atm is 540cal g^(-1) . Calculate DeltaU and DeltaH .

Calculate the K_b for water given latent heat of vaporisation of water 540 Cal//gm .

Latent heat of fusion and vaporisation of water are respectively 80 and 540 Cal g^(-1) . If the boiling point of a solution is 100.1^(@)C , what is its freezing point?

The latent heat of vaporisation of water is 9700 "Cal/mole" and if the b.p.is 100^(@)C , ebullioscopic constant of water is

The latent heat of vaporisation of water is 9700 "Cal/mole" and if the b.p.is 100^(@)C , ebullioscopic constant of water is

Entropy of vaporisation of water at 100^(@)C , if molar heat of vaporisation is 9710 cal mol^(-1) will be