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In a reversible reaction 2NO(2)underset(...

In a reversible reaction `2NO_(2)underset(k_(2))overset(k_(1))iffN_(2)O_(4)`, the rate of disappearance of `NO_(2)` is equal to

A

`(2k_(1))/(k_(2))[NO_(2)]^(2)`

B

`2k_(1) [NO_(2)]^(2)-2K_(2) [N_(2)O_(4)]`

C

`2k_(1)[NO_(2)]^(2) -k_(2) [N_(2)O_(4)]`

D

`(2k_(1)-k_(2))[NO_(2)]`

Text Solution

Verified by Experts

The correct Answer is:
B
`2NO_(2){:(k_(1)),(k_(2)):}N_(2)O_(4)`
In this reaction `NO_(2)` disappears in forward and appears in backward reaction. So rate of disappear once is (consider elementary reaction) `(-d[NO_(2)])/(dt) =2k_(1) [NO_(2)]^(2)-2k_(2)[N_(2)O_(4)]`
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