Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism:
NO...
Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism:
NO(g) + Br2(g) → NOBr2 (g)
NOBr2(g) + NO(g)→2 NOBr
Suppose also k1 ≫ k2. That is, the first step is much faster than the second.
a. Write the balanced chemical equation for the overall chemical reaction.
b. Write the experimentally-observable rate law for the overall chemical reaction.
c. 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.
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