When the following equilibria are disturbed by increasing the pressure, does the concentration of reaction products increase, decrease, or remain the same?2 CO2(g) ⇌ 2 CO(g) + O2(g)

Verified step by step guidance

1. Identify the number of moles of gas on each side of the equilibrium equation. On the left side, there are 2 moles of CO2(g). On the right side, there are 2 moles of CO(g) and 1 mole of O2(g), totaling 3 moles of gas.
2. Apply Le Chatelier's Principle, which states that if a system at equilibrium is subjected to a change in pressure, the system will adjust to counteract that change. Increasing pressure favors the side with fewer moles of gas.
3. Since the left side of the equation has fewer moles of gas (2 moles) compared to the right side (3 moles), increasing the pressure will shift the equilibrium towards the left side.
4. Determine the effect on the concentration of reaction products. As the equilibrium shifts to the left, the concentration of products (CO and O2) will decrease.
5. Conclude that increasing the pressure will result in a decrease in the concentration of the reaction products CO(g) and O2(g).

Key Concepts

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In the context of pressure changes, the system will shift in the direction that reduces the pressure, which typically means favoring the side with fewer gas molecules.

Mole Ratio in Gaseous Reactions

In gaseous reactions, the number of moles of gas on each side of the equilibrium equation is crucial for understanding how changes in pressure affect the system. In the given reaction, there are 2 moles of CO2 on the left and 3 moles (2 CO + 1 O2) on the right, indicating that increasing pressure will favor the formation of CO2, as it has fewer moles of gas.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. While pressure changes can shift the position of equilibrium, the value of K remains constant unless the temperature changes. Understanding K helps predict how concentrations will change in response to disturbances.