For the reaction N_{2(g)} + 3H_{2(g)} rightle | vedclass

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

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Low temperature,high pressure,and catalyst

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(B) $1$. The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 21.9 \ kcal$.
$2$. Since the reaction is exothermic $(\Delta H < 0)$,according to Le Chatelier's principle,low temperature favors the forward reaction.
$3$. The number of moles of gaseous products $(2)$ is less than the number of moles of gaseous reactants $(1+3=4)$. Therefore,high pressure favors the forward reaction (shift towards fewer moles).
$4$. $A$ catalyst is used to increase the rate of the reaction to reach equilibrium faster.
Thus,the favorable conditions are low temperature,high pressure,and the presence of a catalyst.

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 21.9 \ kcal$,which conditions favor the production of ammonia?

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