Answer
The equilibrium constant for this reaction is equal to $1.79 \times 10^{-5}$.
Work Step by Step
1. Write the $K_{eq}$ expression:
$K_{eq} = \frac{[Products]}{[Reactants]} = \frac{[H_2]^2[S_2]}{[H_2S]^2}$
2. Use the given values to calculate the $K_{eq}$ value:
$K_{eq} = \frac{(2.74 \times 10^{-2})^2(7.54 \times 10^{-3})}{(0.562)^2}$
$K_{eq} = 1.79 \times 10^{-5}$
