For the complex formation reaction , the rate of disappearance of the complex is given by: . What is — Chemical Kinetics Chemistry Question
Question
For the complex formation reaction $[Ag(NH_3)_2]^+ \rightleftharpoons Ag^+ + 2NH_3$, the rate of disappearance of the complex is given by: $-\frac{d[Ag(NH_3)_2^+]}{dt} = 2 \times 10^7 \text{ s}^{-1} [Ag(NH_3)_2^+] - 1 \times 10^{13} \text{ L}^2 \text{ mol}^{-2} \text{ s}^{-1} [Ag^+][NH_3]^2$. What is the ratio of the rate constants of the forward and backward reactions ($k_f / k_b$)?
Answer: A
💡 Solution & Explanation
The rate equation is $-\frac{d[Ag(NH_3)_2^+]}{dt} = k_f[Ag(NH_3)_2^+] - k_b[Ag^+][NH_3]^2$. By comparing, $k_f = 2 \times 10^7$ and $k_b = 1 \times 10^{13}$. The ratio $k_f / k_b = \frac{2 \times 10^7}{1 \times 10^{13}} = 2 \times 10^{-6} \text{ mol}^2 \text{ L}^{-2}$.
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