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(C) $1$. The reaction involves a change in the total number of moles of gaseous species: $4 	ext{ moles}$ on the reactant side and $1 	ext{ mole}$ o

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Both temperature and pressure

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(C) $1$. The reaction involves a change in the total number of moles of gaseous species: $4 	ext{ moles}$ on the reactant side and $1 	ext{ mole}$ on the product side. According to Le Chatelier's principle, a change in pressure will shift the equilibrium.$2$. Since the reaction is exothermic ($\Delta H = -q 	ext{ kJ}$, where $q > 0$), a change in temperature will also shift the equilibrium.$3$. $A$ catalyst only increases the rate of both forward and backward reactions equally and does not affect the equilibrium position or the amount of product formed.$4$. Therefore, the amount of product is affected by both temperature and pressure.

For the following gaseous reversible reaction: $3A_{(g)} + B_{(g)} \rightleftharpoons A_3B_{(g)}$ $(\Delta H = -q \text{ kJ})$. The amount of product $A_3B_{(g)}$ is affected by . . . . . .

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