The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO₂(g) NaHCO₃(s) ΔH°_rxn

Question

The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO₂(g)

The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO<sub>2</sub>(g) NaHCO<sub>3</sub>(s) ΔH°<sub>rxn</sub> < 0 Which, if any, of the following actions will decrease the concentration of CO<sub>2</sub> gas present at equilibrium? A) adding N<sub>2</sub> gas to double the pressure B) adding more solid NaOH C) increasing the volume of the container D) lowering the temperature E) None of these choices are correct.

NaHCO₃(s) ΔH°_rxn < 0
Which, if any, of the following actions will decrease the concentration of CO₂ gas present at equilibrium?

Quizplus · Accepted Answer

According to Le Chatelier's principle, when a system at equilibrium is subjected to a change in temperature, it will shift in the direction that absorbs or releases heat to counteract the change. The reaction is exothermic, so decreasing the temperature will shift the equilibrium to favor the production of more heat, which will be achieved by decreasing the concentration of CO₂ gas. Therefore, lowering the temperature will decrease the concentration of CO₂ gas present at equilibrium. Adding more CO₂ gas (A) will actually shift the equilibrium to favor the production of more NaHCO₃, while adding more solid NaOH (B) or increasing the volume of the container (C) will have no effect on the concentration of CO₂ gas.

The Following Reaction Is at Equilibrium at a Pressure of 1