In an equilibrium reaction, the rate constants of the forward and backward reactions are 3.2×10−4mol−1dm3s−1 and 1.2×10−5mol−1dm3s−1, respectively. The equilibrium constant of the reaction is

In an equilibrium reaction, the rate constants of the forward and backward reactions are $3.2×{10}^{-4}{\mathrm{mol}}^{-1}{\mathrm{dm}}^{3}{\mathrm{s}}^{-1}$ and $1.2×{10}^{-5}{\mathrm{mol}}^{-1}{\mathrm{dm}}^{3}{\mathrm{s}}^{-1}$, respectively. The equilibrium constant of the reaction is

1. A

0.25

2. B

0.37

3. C

3.7

4. D

26.7

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Solution:

${K}_{\mathrm{eq}}={k}_{\mathrm{f}}/{k}_{\mathrm{b}}=3.2×{10}^{-4}{\mathrm{mol}}^{-1}{\mathrm{dm}}^{3}{\mathrm{s}}^{-1}/1.2×{10}^{-5}{\mathrm{mol}}^{-1}{\mathrm{dm}}^{3}{\mathrm{s}}^{-1}=26.7$

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