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The standard enthalpies of formation of `H_(2)O_(2(l)) and H_(2)O_((l)) " are " -187.8 kJ "mole"^(-1) and -285.8 kJ "mole"^(-1)` respectively. The `Delta H^(0)` for the decomposition of one mole of `H_(2)O_(2(l)) " to " H_(2)O_((l)) and O_(2(g))` is

A

`-473.6 kJ. "mole"^(-1)`

B

`-98.9 kJ "mole"^(-1)`

C

`+473.6 kJ "mole"^(-1)`

D

`+187.8 kJ "mole"^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
B
The given reaction is `H_(2)O_(2(l)) rarr H_(2)O_((l)) + (1)/(2) O_(2(g))`
`Delta H= Sigma` Heat of formation of products `-Sigma` Heat of formation of reactants `=(-285.8) + (0) - (-187.8) = -98`
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AAKASH SERIES-CHEMICAL THERMODYNAMICS-LECTURE SHEET (EXERCISE-II) (LEVEL - I(MAIN) STRAIGHT OBJECTIVE TYPE QUESTIONS)
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