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In gaseous reactions important for under...

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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H_(2)O and O atom react in upper atmosphere bimolecularly to form two OH radicals. DeltaH for the reaction is 72 kJ at 500K and energy of activation is 77kJ mol^(-1) . Estimate E_(a) for bimolecular recombination of two OH radicals to form H_(2)O and O atom.

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  • In gaseous reactions important for the understanding of the upper atomoshphere H_2O and O react bimolecularly to form two OH radicals . DeltaH for this reaction is 72 kJ mol^(-1) at 500 K and E_a is 77 kJ mol^(-1) then E_a for the bimolecular recombination of two OH radicals to form H_2O to O is:

    A
    `3 kJ mol^(-1)`
    B
    `4 kJ mol^(-1)`
    C
    `5 kJ mol^(-1)`
    D
    `7 kJ mol^(-1)`

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    A
    `3 kJ "mol"^(-1)`
    B
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    D
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  • H_(2)O and O-atom react in upper atmosphere bimolecularly to form two OH radicals. DeltaH for the reaction is 72 kJ at 500 K and energy of activation is 77 kJ "mol"^(-1).E_(a) for bimolecular recombination of two OH radicals to form H_(2)O and O-atom, will be

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