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One mole of ice is converted into water ...

One mole of ice is converted into water at 273 K. The entropies of `H_2O_((s)) and H_2O_((l))` are `38.20 and 60.01 J mol^(-1)K^(-1)` respectively. The enthalpy change for the conversion is 

A

`5951.4 J//"mol"`

B

`595.14 J//"mol"`

C

`-5951.4 J//"mol"`

D

None of these

Text Solution

Verified by Experts

The correct Answer is:
A
At equilibrium `therefore " "DeltaH=T.DeltaS`
`H_(2)O(s)rarrH_(2)O(l)`
`DeltaS=S_(H_(2)O(l))-S_(H_(2)O(s))=21.8 J//"mol-K"`
`DeltaH=273 xx (21.8)=5951.4 J//"mol"`
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