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The formation of product $P$ occurs in a two-step reaction.

Step 1: $A + B$ $\rightleftharpoons$ $C$ (fast) $\quad K_{eq}$ = $1.5 \times 10^{-5}$

Step 2: $C + B$ $\rightleftharpoons$ $A + P$ (slow) $\quad K_{eq}$ = $4.4 \times {10^{-11}}$

Which of the following is the $K_{eq}$ for the overall reaction that represents the formation of $P$?

A

$6.6 \times10^{-16}$

B

$1.50 \times10^{-5}$

C

$3.41 \times10^{5}$

D

$6.6 \times10^{16}$

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