For the reaction: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, $\Delta H = -92\,kJ\,mol^{-1}$. Which condition would shift the equilibrium to the right to produce more ammonia?

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Increasing pressure and decreasing temperature. The forward reaction is exothermic, so decreasing temperature favours the forward reaction by Le Chatelier's principle. The forward reaction also reduces the number of moles of gas from 4 to 2, so increasing pressure shifts equilibrium to the right where fewer gas moles exist. Together, high pressur

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A) Increasing temperature and decreasing pressure

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B) Decreasing pressure and adding a catalyst

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C) Increasing pressure and decreasing temperature

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D) Decreasing temperature and removing the catalyst

For the reaction: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, $\Delta H = -92\,kJ\,mol^{-1}$. Which condition would shift the equilibrium to the right to produce more ammonia?

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