Problem: The reaction described by this equation: O3(g) + NO(g) ----> O2(g) + NO2(g)has the following rate law at 310 K.rate of reaction = k [O3][NO]k = 3.0 x 106 M-1s-1Given that [O3] = 7.0 x 10-4 M and [NO] = 8.0 x 10-5 M at t=0, calculate the rate of the reaction at t=0. _______M/sWhat is the overall order of this reaction? 0, 1, 2, or 3?Explain the answer.

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A) Given that [O3] = 7.0 x 10-4 M and [NO] = 8.0 x 10-5 M at t=0, calculate the rate of the reaction at t=0. _______M/s

k = 3.0 x 106 M-1s-1


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Problem Details

The reaction described by this equation: O3(g) + NO(g) ----> O2(g) + NO2(g)

has the following rate law at 310 K.

rate of reaction = k [O3][NO]

k = 3.0 x 106 M-1s-1

Given that [O3] = 7.0 x 10-4 M and [NO] = 8.0 x 10-5 M at t=0, calculate the rate of the reaction at t=0. _______M/s

What is the overall order of this reaction? 0, 1, 2, or 3?

Explain the answer.

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