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InterviewSolution
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The rate constant for the decompoistion of a certain reaction is described by the equation: `log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T)` A two-step mechanism has been suggested for the reaction of nitric oxide and bromine: `NO(g) + Br_(2)(g) overset(k_(1))rarr NOBr_(2)(g)` `NOBr_(2)(g)+NO(g) overset(k_(2))rarr 2NOBr(g)` The observed rate law is, rate `= k[NO]^(2)[Br_(2)]`. Hence, the rate-determining step isA. `NO(g)+Br_(2)(g) rarr NOBr_(2)(g)`B. `NOBr_(2)(g)+NO(g) rarr 2NOBr(g)`C. `2NO(g) + Br_(2)(g) rarr 2NOBr(g)`D. None of these |
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Answer» Correct Answer - B `NO(g)+Br_(2)(g) overset(k_(1))hArr NOBr_(2)(g)` …(i) `NOBr_(2)(g)+NO(g)underset(RDA)overset(k_(2))rarr 2NOBr(g)` …(ii) `:. Rate = k_(2)[NOBr_(2)][NO]` …(iii) Since `NOBr_(2)` is the reactive intermediate, so its concentration is determined form step (i). `:. k_(1) or k_(eq) = ([NOBr_(2)])/([NO][Br_(2)])` or `[NOBr_(2)] = k_(1)[NO][Br_(2)]` Substitute the `[NOBr_(2)]` in step (iii), `:. Rate = k_(1)k_(2)[NO]^(2)[Br_(2)] = K[NO]^(2)[Br_(2)]` |
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