(a)Show that the rate law is $\frac{\mathrm{d}[\mathrm{BD}]}{\mathrm{dt}}=\frac{\mathrm{k}_{2} \cdot \mathrm{k}_{1} \cdot[\mathrm{CB}]^{2}}{\mathrm{k}_{-1} \cdot[\mathrm{CB}]+\mathrm{k}_{2}}$
(b)The apparent first-order rate constant, $\mathrm{k_{app}} = \dfrac{\mathrm{k_2 \cdot k_1 \cdot [CB]}}{\mathrm{k_{-1} \cdot [CB] + k_2}}$. At the CB concentration of $1 \times 10^{-5}$ mol ____ ratio $\dfrac{\mathrm{k_2}}{\mathrm{k_{-1}}}$.
Answer
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