While `1mol` of ice melts at `0^(@)C` and at constant pressure of `1atm, 1440 cal` of heat are absorbed by the system. The molar volume of ice and water are `0.0196` and `0.0180L` respectively. Calculate `DeltaH` and `DeltaU`.

When1 mole of ice melt at 0^(@) C and at constant pressure of 1 atm . 1440 calories of heat are absorbed by the system. The molar volumes of ice and water are 0.0196 and 0.0180 litres respectively. Calculate DeltaH and DeltaE for the reaction.

When1 mole of ice melt at 0^(@) C and at constant pressure of 1 atm . 1440 calories of heat are absorbed by the system. The molar volumes of ice and water are 0.0196 and 0.0180 litres respectively. Calculate DeltaH and DeltaE for the reaction.

4 KJ of heat is absorbed when 1 mole of ice melts at 0^(@)C and at constant pressure 1 atm . If molar volume of ice and water are 19 ml and 18 ml respectively, then [Take 1 atm=10^(5)Pa ]

1 mol e of ice melts at 0^(@)C and constant pressure of 1 atm by absorbing 1.44kcal heat . The density of ice 0.918 g//Ml and of water 1g//mL respectively. The two values of DeltaH and DeltaU differ by :

When 1 g of ice at 0^(@)C melts to form 1 g of water at 0^(@)C then, is the latent heat absorbed by the ice or given out by it?