Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism:step elementary reaction rate constant1 →+NOgBr2gNOBr2g k12 →+NOBr2gNOg2NOBrg 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 reaction between nitric oxide and bromine proceeds by the following mechanism:step elementary reaction rate constant1 →+NOgBr2gNOBr2g k12 →+NOBr2gNOg2NOBrg 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:
Step 1: NO(g) + Br2(g) → NOBr2(g) Step 2: NOBr2(g) + NO(g) → 2NOBr(g)
Adding these together, we get:
NO(g) + Br2(g) + NO(g) → NOBr2(g) + 2NOBr(g)
Simplifying, we get:
2NO(g) + Br2(g) → 2NOBr(g)
The rate law for the overall reaction can be written based on the slowest step (rate-determining step), which is the first step in this case. Since the first step is a bimolecular reaction involving NO and Br2, the rate law is:
rate = k1[NO][Br2]
Note: The rate law does not include the concentration of the intermediate (NOBr2) because the concentration of intermediates is generally not experimentally observable.
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