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

If `DeltaH_(f)^(@)` for `H_(2)O_(2)(l) and H_(2)O(l)` are -188kJ and `mol^(-1)` and -286 kJ `mol^(-1)`, what will be the enthalpy change of the reaction `2H_(2)O_(2)(l)to2H_(2)O(l)+O_(2)(g)`?

A

`-196 kJ cdot" mol"^(-1)`

B

`-19.6 kJ cdot" mol"^(-1)`

C

`-1960 kJ cdot" mol"^(-1)`

D

`-1.96 kJ cdot" mol"^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
A
`Delta H _("reaction") =2 Delta _(f)H^(0)(H_(2)O)-2Delta_(f)H^(0)(H_(2)O_(2))=2(-286)-2(-188)-2(-188)=-196 kJ`
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