For the reaction , the equilibrium constant . At a certain instant, the concentrations are , , and . — Chemical Equilibrium Chemistry Question
Question
For the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, the equilibrium constant $K_c = 1.7 \times 10^2$. At a certain instant, the concentrations are $[N_2] = 0.42\text{ M}$, $[H_2] = 0.20\text{ M}$, and $[NH_3] = 0.10\text{ M}$. Which of the following correctly predicts the direction of the reaction?
Answer: B
💡 Solution & Explanation
The reaction quotient $Q_c$ is calculated as $Q_c = \frac{[NH_3]^2}{[N_2][H_2]^3} = \frac{(0.10)^2}{(0.42)(0.20)^3} = \frac{0.01}{0.42 \times 0.008} \approx 2.976$. Since $Q_c \approx 2.976$ is much less than $K_c$ ($1.7 \times 10^2$), the reaction will proceed from left to right (forward direction) to reach equilibrium.
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