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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.

A

`DeltaH=720` J

B

`DeltaH = 1440` cal

C

`DeltaH=1.4 Kcal`

D

`DeltaH=0`

Text Solution

Verified by Experts

The correct Answer is:
B
`H_(2)O(s) to H_(2)O (l), DeltaH = 1440` cal
`DeltaH =~ DeltaU` for solids and liquids.
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