Suppose the decomposition of nitryl chloride proceeds by the following mechanism:step elementary reaction rate constant1 NO2Cl(g) → NO2(g) + Cl(g) k12 Cl(g) + NO2Cl(g) → NO2(g) + Cl2(g) k2Suppose 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. =ratek 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.
Question
Suppose the decomposition of nitryl chloride proceeds by the following mechanism:step elementary reaction rate constant1 NO2Cl(g) → NO2(g) + Cl(g) k12 Cl(g) + NO2Cl(g) → NO2(g) + Cl2(g) k2Suppose 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. =ratek 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.
Solution
The balanced chemical equation for the overall chemical reaction is:
2NO2Cl(g) → 2NO2(g) + Cl2(g)
The rate law for the overall chemical reaction is determined by the slowest step, which is the first step in this case. Therefore, the rate law is:
rate = k1[NO2Cl]
The rate constant k for the overall reaction is equal to the rate constant of the slowest step, which is k1 in this case. Therefore, k = k1.
Note: Since the first step is the slowest and determines the rate, the rate constants for the reverse reactions and the second step (k-1, k-2, and k2) do not appear in the rate law or the expression for the overall rate constant.
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