Consider the equilibrium {N_2}_{(g)} + 3{H_2} | vedclass

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(A) According to Le Chatelier's principle,for an exothermic reaction $(\Delta H < 0)$,a decrease in temperature favors the forward reaction to produce

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Decrease of temperature and increase of pressure

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(A) According to Le Chatelier's principle,for an exothermic reaction $(\Delta H Since the number of moles of gaseous products $(2 \ mol)$ is less than the number of moles of gaseous reactants $(1 + 3 = 4 \ mol)$,an increase in pressure shifts the equilibrium towards the side with fewer moles,which is the product side.Therefore,the maximum yield of ammonia is obtained by decreasing the temperature and increasing the pressure.

Consider the equilibrium ${N_2}_{(g)} + 3{H_2}_{(g)} \rightleftharpoons 2N{H_3}_{(g)}$,$\Delta H = -93.6 \ kJ$. The maximum yield of ammonia is obtained by:

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