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DeltaH(f)^(@) of water is -285.5 KJ "mol...

`DeltaH_(f)^(@)` of water is -285.5 KJ `"mol"^(-1)`. If enthalpy of neutralisation of monoacid strong base is -57.3 KJ `"mol"^(-1) , DeltaH_(f)^(@)` of `OH^(-)` ion will be

A

`-228.5 kJ mol^(-1)`

B

`228.5 kJ mol^(-1)`

C

`114.25 kJ mol^(-)`

D

`-114.25 kJ mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
A
`H_(2)+1/2 O_(2) rarr H_(2)O" "DeltaH=-285.8`
Target reaction `H^(+)+OH^(-) rarr H_(2)O" "DeltaH=-57.3`
`Delta=-57.3=[-285.8-0-x]" "x=DeltaH_(f)^(@)` of `OH^(-)`
`x=-228.5" kJ mol"^(-1)`
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