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In gaseous reactions important for understanding of the upper atmosphere `H_(2)O and O` react bimolecularly to form two OH radicals. `Delta H` for this reaction is 72kJ/mol at `500 K and E_(a) = 77 kJ//mol`, then `E_(a)` for two bimolecular recombination of 2OH radicals to form `H_(2)O & O` is

A

`3" kJ mol"^(-1)`

B

`4" kJ mol"^(-1)`

C

`5" kJ mol"^(-1)`

D

`7" kJ mol"^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
C
As `Delta H` is positive, therefore reaction is endothermic This is the energy profile diagram for an endothermic reaction. Now when the products is converted back to reactant the energy of activation is x as shown in fig. Evidently `x=E_(a) -Delta H`
`=(77-72) =5" kJ mol"^(-1)`
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