Question

Suppose the decomposition of ozone proceeds by the following mechanism: step | elementary reaction | rate constant 1 | O3(g) ? O2(g) + O(g) | k1 2 | O3(g) + O(g) ? 2 O2(g) | k2 Suppose also k1 ? k2. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = k Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. k =

          Suppose the decomposition of ozone proceeds by the following mechanism:

step | elementary reaction | rate constant
1 | O3(g) ? O2(g) + O(g) | k1
2 | O3(g) + O(g) ? 2 O2(g) | k2

Suppose also k1 ? k2. That is, the first step is much slower than the second.

Write the balanced chemical equation for the overall chemical reaction:

Write the experimentally-observable rate law for the overall chemical reaction.
Note: your answer should not contain the concentrations of any intermediates.
rate = k

Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.
k =

Suppose the decomposition of ozone proceeds by the following mechanism:

step | elementary reaction | rate constant
1 | O3(g) ? O2(g) + O(g) | k1
2 | O3(g) + O(g) ? 2 O2(g) | k2

Suppose also k1 ? k2. That is, the first step is much slower than the second.

Write the balanced chemical equation for the overall chemical reaction:

Write the experimentally-observable rate law for the overall chemical reaction.
Note: your answer should not contain the concentrations of any intermediates.
rate = k

Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.
k =

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