When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s) + H₂(g) ⇌ H₂O(g) + Cu(s) $\Delta$Hº_rxn = -2.0 kJ/mol

Question

Quizplus · Accepted Answer

Le Chatelier's principle states that a system at equilibrium will shift to counteract any stress that is applied to it. In this case, decreasing the temperature would shift the equilibrium to favor the exothermic reaction (the production of H₂O and Cu). This is because the forward reaction (from left to right) is exothermic and the reverse reaction (from right to left) is endothermic. Therefore, by decreasing the temperature, we are removing some of the heat from the system, which helps to shift the equilibrium to favor the exothermic reaction. The other answer choices either do not apply to this situation (such as options A and B) or would have little to no effect on the equilibrium (such as options D and E).

When the Substances in the Equation Below Are at Equilibrium Δ\DeltaΔ

When the Substances in the Equation Below Are at Equilibrium $\Delta$