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The reaction described by this equation O_3(g) + NO(g) rightarrow O_2(g) + NO_2(g) the following rate law at 310 K. rate of reaction = k[O_3][NO] k = 3.0 times 10^6 M^-1 middot s^-1 Given that [O_3] = 5.0 times 10^-4 M and [NO] = 8.0 times 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 3
The reaction described by this equation O_3(g) + NO(g) rightarrow O_2(g) + NO_2(g) the following rate law at 310 K. rate of reaction = k[O_3][NO] k = 3.0 times 10^6 M^-1 middot s^-1 Given that [O_3] = 5.0 times 10^-4 M and [NO] = 8.0 times 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 3
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Patrina SchowalterLv2
18 Oct 2019
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