When the substances in the equation below are at equilibrium at pressure P and temperature T, how can the equilibrium be shifted to favor the products? CuO(s) + H₂(g) Cu(s) + H₂O(g)
Change in enthalpy = -2.0 kJ.

Question

When the substances in the equation below are at equilibrium at pressure P and temperature T, how can the equilibrium be shifted to favor the products? CuO(s) + H₂(g)

Cu(s) + H₂O(g)
Change in enthalpy = -2.0 kJ.

Quizplus · Accepted Answer

According to Le Chatelier's principle, if we decrease the temperature, the equilibrium will shift in the direction of the reaction that produces heat, which in this case is the forward reaction. Therefore, the equilibrium will shift to favor the products, Cu(s) and H₂O(g).

When the Substances in the Equation Below Are at Equilibrium