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Anton [14]
3 years ago
10

g Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant That is

, the first step is much faster 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. 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.

Chemistry
1 answer:
PIT_PIT [208]3 years ago
5 0

Answer:

Check the explanation

Explanation:

Kindly check the attached image below to see the step by step explanation to the question above.

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