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13 Dec 2019
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.
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.
Beverley SmithLv2
17 Dec 2019