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In gaseous reaction, important for the understanding of the upper atmosphere `H_(2)O` and O react bimolecularly to from two OH readicals. `DeltaH` for this reaction is 72 kJ at 500 K and `E_(a)` is 77 kJ `"mol"^(-1)`, then `E_(a)` for the bimolecular recombination of two OH readicals to form `H_(2)O` and O is :

A

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

B

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

C

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

D

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

Text Solution

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The correct Answer is:
C
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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

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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.

Water and oxygen atoms react in upper atmospheric level bimolecularly to form two OH radicals having heat of reaction 72 kJ at 400 K and energy of activation being 77 kJ mol^(-1) . Calculate the E_(a) for bimolecular combination of two OH radicals to form H_(2)O and O -atom.

There is formation of H_(2)O_(2) in the upper atomsphere. H_(2)O + O rarr 2OH rarr H_(2)O_(2) Delta H = 72 kJ mol^(-1) , E_(a) = 77 kJ mol^(-1) What will be the E_(a) for bimolecular recombination of two OH radicals to form H_(2)O and O in kJ.

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