For the reaction N_2 + 3H_2 rightleftharpoons | vedclass

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(B) $1$. The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 21.9 \, kcal$.
$2$. The reaction is exothermic $(\Delta H < 0

Vedclass · Accepted Answer

Low temperature,high pressure

Vedclass · Answer

(B) $1$. The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 21.9 \, kcal$.
$2$. The reaction is exothermic $(\Delta H < 0)$,so according to Le Chatelier's principle,a low temperature favors the forward reaction (production of $NH_3$).
$3$. The number of moles of gaseous reactants is $1 + 3 = 4$,and the number of moles of gaseous products is $2$. Since the forward reaction involves a decrease in the number of moles,high pressure favors the forward reaction.
$4$. Therefore,low temperature and high pressure are the ideal conditions for the production of ammonia.

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3 + 21.9 \, kcal$,under which conditions is the production of ammonia favored according to Le Chatelier's principle?

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