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Heat of Reaction

Heat of forma...

Question

Heat of formation of $H_{2} O$ is $- 188$ kJ/mol and $H_{2} O_{2}$ is $- 286$ kJ/mol. The enthalpy change for the following reaction is:
$2 H_{2} O_{2} \to 2 H_{2} O + O_{2}$

196

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- 196

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984

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Solution

The correct option is C $- 196$ kJ
$Δ H_{r e a c t i o n} = (\sum H_{p r o d u c t s}) - (\sum H_{r e a c t a n t s})$
$Δ H_{r e a c t i o n} = [(Δ H_{O_{2}}) + (Δ H_{H_{2} O})] - [Δ H_{H_{2} O_{2}}]$
$Δ H_{O_{2}} = 0, Δ H_{H_{2} O} = - 286 K J p e r m o l e, Δ H_{H_{2} O_{2}} = - 188 K J p e r m o l e$
put the values ,
$Δ H_{r e a c t i o n} = - 196 K J p e r m o l e$

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