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 $3.2 \times 10^{- 4} {mol}^{- 1} {dm}^{3} s^{- 1}$ and $1.2 \times 10^{- 5} {mol}^{- 1} {dm}^{3} s^{- 1}$ , respectively. The equilibrium constant of the reaction is

A
0.25
B
0.37
C
3.7
D
26.7

Solution:

$K_{eq} = k_{f} / k_{b} = 3.2 \times 10^{- 4} {mol}^{- 1} {dm}^{3} s^{- 1} / 1.2 \times 10^{- 5} {mol}^{- 1} {dm}^{3} s^{- 1} = 26.7$

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