Consider 4 kg of water at `100^@C`. How much amount of heat is required to convert it into steam ?

How much water is required for drinking ?

Assume that heat capacity of H_(2) O to be 4.2 xx 10^(3) J kg ^ (-1) K^(-1) and the latent heat of vapourisation of H_(2) O to be 22.5 xx 10^(5) J kg^(-1) . The amount of heat in joule required to heat 1 kg of water from 50^(@)C to 100^(@)C and then to convert into steam at 100^(@)C is

The temperature of water at 100^@ C remains constant till all the water is converted into -

A swimmer coming out from a pool is covered with a film of water weighing about 18g. How much heat must be supplied to evaporate this water at 298 K? Calculate the internal energy of vaporisation at 100^@C . DeltaH_(vap)^@ for water at 373K = 40.66 kJ mol^(-1)