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The decomposition of NO2 at 400K proceed...

The decomposition of `NO_2` at 400K proceeds at a rate of `5.4 xx 10^-5 mol L^-1s^-1` when `[NO_2] = 0.01 mol L^-1`.
`2NO_2(g) rArr 2NO(g) + O_2(g)`
What is the rate law when observed rate is `1.35 xx 10^-5 mol L^-1 s^-1` at `[NO_2] = 0.005 mol L^-1`?

A

K[`NO_2]`

B

K[`NO_2]^2`

C

K[`NO_2]^3`

D

K[`NO_2]^0`

Text Solution

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The correct Answer is:
B
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