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) ΔHº_rxn = -2.0 kJ/mol

Question

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) ΔHº_rxn = -2.0 kJ/mol

Quizplus · Accepted Answer

According to Le Chatelier's principle, when a system at equilibrium is subjected to a stress, the system will shift in the direction that tends to counteract that stress. In this case, decreasing the temperature will favor the products because the reaction is exothermic (ΔHº_rxn is negative). By decreasing the temperature, the system will try to produce more heat by favoring the side with fewer moles of gas (the products). Therefore, the equilibrium will shift to the right, favoring the products. The other options (A, B, D, and E) do not have any effect on the equilibrium position because they do not affect the temperature or the concentration of the reactants or products.

When the Substances in the Equation Below Are at Equilibrium,at