Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. c. CaCO₃(s) ⇌ CaO(s) + CO₂(g) (volume is increased)

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 itself to counteract the change and restore a new equilibrium. This principle is crucial for predicting how a system will respond to changes in concentration, temperature, or pressure.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For gaseous reactions, changes in volume affect the partial pressures of the gases involved, which in turn influences the position of equilibrium.

Effect of Volume Change on Gaseous Equilibria

In reactions involving gases, increasing the volume decreases the pressure. According to Le Chatelier's Principle, the equilibrium will shift toward the side with more moles of gas to counteract the decrease in pressure. In the given reaction, the products side has one mole of gas (CO2), while the reactants side has none, indicating a shift to the right when volume is increased.