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The Haber process is the name given for the industrial conditions for synthesizing ammonia:

$$N_{2 (g)} \ + 3 \ H_{2 (g)} \rightleftharpoons 2 \ NH_{3 (g)} \ \ \ \ \ \ \ K = 4.46 \times 10^{-3}$$

If $[N_2] = 2.00 \text{ M}$, $[H_2] = 2.00 \text{ M}$ and $[NH_3] = 7.00 \text{ M}$, which of the following can be concluded about the reaction at equilibrium?

A

Yes, the reaction is at equilibrium and has stopped.

B

No, the reaction is not at equilibrium and must proceed forward to reach equilibrium.

C

No, the reaction is not at equilibrium and must proceed in reverse to reach equilibrium.

D

Yes, the reaction is at equilibrium, indicating the forward and reverse reactions are continuing at equal rates.

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