Suppose the formation of nitrosyl chloride proceeds by the following mechanism:step elementary reaction rate constant1 →+NOgCl2gNOCl2g k12 →+NOCl2gNOg2NOClg 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.
Question
Suppose the formation of nitrosyl chloride proceeds by the following mechanism:step elementary reaction rate constant1 →+NOgCl2gNOCl2g k12 →+NOCl2gNOg2NOClg 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.
Solution
The overall balanced chemical equation for the reaction can be obtained by adding the two elementary reactions together:
NO(g) + Cl2(g) -> NOCl2(g) (Step 1) NOCl2(g) + NO(g) -> 2NOCl(g) (Step 2)
2NO(g) + Cl2(g) -> 2NOCl(g) (Overall Reaction)
The rate law for the overall reaction can be determined by considering the slowest step (rate-determining step) in the reaction mechanism, which is the first step in this case. Since the rate of the reaction is determined by the slowest step, the rate law is written in terms of the reactants of this step.
Therefore, the rate law for the overall reaction is:
rate = k1[NO][Cl2]
This rate law indicates that the rate of the reaction is directly proportional to the concentration of NO and Cl2. The rate constant, k1, is a proportionality constant that depends on the temperature of the reaction.
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