Chemical Kinetics and Nuclear ChemistryMedium
Question
For hypothetical reaction A → B takes place according to
$$A\overset{\quad K_{1}\quad}{\leftleftarrows}C\left( \text{fast} \right) $$$A + C\overset{\quad K_{2}\quad}{\rightarrow}B\left( \text{slow} \right)$
The rate of reaction is (K1 is equilibrium constant)
Options
A.K2[B][C]
B.K1K2[A]
C.K1K2[A]2
D.K1[B][C]
Solution
$r = K_{2}\lbrack A\rbrack\lbrack C\rbrack\text{ and }K_{1} = \frac{\lbrack C\rbrack}{\lbrack A\rbrack}$
$\therefore r = K_{1}K_{2}\lbrack A\rbrack^{2}$
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