When1 mole of ice melt at 0^(@) C and at...

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.

`DeltaH=720` Joule

`DeltaH=1440` cal

`DeltaH=1.4` Kcal

`DeltaH=0`

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The correct Answer is:

`H_(2)O(s) rarr H_(2)O(l) , DeltaH = 1440 "cal"`
`DeltaH~= DeltaU` for solids and liquids

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