Calculate the entropy change `(DeltaS)` when `1 mol` of ice at `0^(@)C` is converted into water at `0^(@)C`. Heat of fusion of ice at `0^(@)C` is `1436 cal` per mol.

Calculate the amount of heat energy to be supplied to convert 2 kg of ice at 0^@C completely into water at 0^@C if latent heat of fusion for ice is 80 cal/g.

Calculate the amount of heat energy to be supplied to convert 4 kg of ice at 0^@C completely into water at 0^@C if latent heat of fusion for ice is 80 cal/g.

Calculate the amount of heat required to convert5g of ice of 0^(@)C into water at 0^(@)C . ( Specific latent heat of fusion of ice 80 cal //g )

100 gram of ice at 0^@C is converted into water vapour at 100^@C Calculate the change in entropy.

Calculate the entropy change when 20.0 g of ice changes to liquid water at 0°C. The heat of fusion is 80.0 cal g^(-1) .

What is the entropy change (in JK^(-1)mol^(-1) ) when one mole of ice is converted into water at 0^(@)C ? (The enthalpy change for the conversion of ice to liquid water is 6.0KJmol^(-1) at 0^(@)C )

What is the entropy change (in JK^(-1)mol^(-1) ) when one mole of ice is converted into water at 0^(@)C ? (The enthalpy change for the conversion of ice to liquid water is 6.0KJmol^(-1) at 0^(@)C )