Question

Ammonia is synthesized via the following chemical reaction: N_{2(g)}+3 H_{2(g)} \leftrightarrow 2 N H_{3(g)} \text { where } K=6.01 \times 10^{-2} Given the following initial conditions, determine if the given concentrations represent an equilibrium. If not, predict the direction in which the reaction will proceed to reach equilibrium. [3 marks T] \left[\mathrm{NH}_{3(\mathrm{~g})}\right]=2.00 \times 10^{-4} \mathrm{~mol} / \mathrm{L} \left[\mathrm{N}_{2(\mathrm{~g})}\right]=1.50 \times 10^{-5} \mathrm{~mol} / \mathrm{L} \left[\mathrm{H}_{2}(\mathrm{~g})\right]=3.54 \times 10^{-1} \mathrm{~mol} / \mathrm{L}

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