Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism:step elementary reaction rate constant1 NO2(g) + O3(g) → NO3(g) + O2(g) k12 NO3(g) + NO2(g) → N2O5(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. =k
Question
Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism:step elementary reaction rate constant1 NO2(g) + O3(g) → NO3(g) + O2(g) k12 NO3(g) + NO2(g) → N2O5(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. =k
Solution
The balanced chemical equation for the overall chemical reaction is:
NO2(g) + O3(g) + NO2(g) → N2O5(g) + O2(g)
The experimentally-observable rate law for the overall chemical reaction is:
rate = k[NO2]^2[O3]
This is because the rate of the reaction is determined by the slowest step, which is the first step. The rate law is proportional to the concentration of the reactants in the slow step, raised to their stoichiometric coefficients.
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 is:
k = k1 * k2 / (k-1 + k2)
This is because the overall rate constant is the product of the rate constants of the individual steps, divided by the sum of the rate constants for the reverse reactions. However, since k1 is much smaller than k2, we can approximate that k ≈ k1. This is because the reaction is essentially controlled by the slowest step, which is the first step with rate constant k1.
Similar Questions
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