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If DeltaH(f)^(@) for H(2)O(2) and H(2)O ...

If `DeltaH_(f)^(@)` for `H_(2)O_(2)` and `H_(2)O` are `-188` kJ/mole and `-286` kJ/mole, what will be the enthalpy change of the reaction `H_(2)O_(2) rarr H_(2)O+1/2 O_(2)`

A

`-196`kJ/mole

B

146kJ/mole

C

`-494`kJ/mole

D

`-98` kJ/mole

Text Solution

Verified by Experts

The correct Answer is:
A
`H_(2)(g) + O_(2)(g) rarr H_(2)O_(2)(l) " " Delta H= -188`
`H_(2)(g) + (1)/(2) O_(2)(g) rarr H_(2)O(l) Delta H= -286`
By Lavoisier and Laplace Law:
`2H_(2)O_(2)(l) rarr 2H_(2)(g) + 2O_(2)(g), Delta H= +376`
`2H_(2)(g) + O_(2)(g) rarr 2H_(2)O(l), Delta H= -572`
Adding the above two equations by using Hess' Law :
`2H_(2)O_(2)(l) rarr 2H_(2)O(l) + O_(2) (g) Delta H= -196`
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