The reaction 2A + B $\rightarrow$ D + E has the rate law,rate = a[A]²[B]/(b + c[A]) where a,b,and c are constants.The following mechanism has been proposed for this reaction.
A + B
k₁,k_-1
$f$
I
I + A $\rightarrow$ D + E
k₂
I is an unstable intermediate present in minute concentrations.Show that this mechanism leads to the observed rate law and evaluate the constantsa,b,and c in terms of the rate constants k₁,k_-1,and k₂.

Question

The reaction 2A + B

\rightarrow

D + E has the rate law,rate = a[A]²[B]/(b + c[A]) where a,b,and c are constants.The following mechanism has been proposed for this reaction.
A + B
k₁,k_-1

f

I
I + A

\rightarrow

D + E
k₂
I is an unstable intermediate present in minute concentrations.Show that this mechanism leads to the observed rate law and evaluate the constantsa,b,and c in terms of the rate constants k₁,k_-1,and k₂.

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The Answer of The reaction 2A + B $\rightarrow$ D + E has the rate law,rate = a[A]²[B]/(b + c[A]) where a,b,and c are constants.The following mechanism has been proposed for this reaction. A + B k₁,k_-1 $f$ I I + A $\rightarrow$ D + E k₂ I is an unstable intermediate present in minute concentrations.Show that this mechanism leads to the observed rate law and evaluate the constantsa,b,and c in terms of the rate constants k₁,k_-1,and k₂.

The Reaction 2A + B →\rightarrow→ D + E Has the Rate Law,rate = A[A]2[B]/(b

The Reaction 2A + B $\rightarrow$ D + E Has the Rate Law,rate = A[A]²[B]/(b