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. a. CO(g) + H₂O( g) ⇌ CO₂(g) + H₂(g) (volume is decreased)

Key Concepts

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This principle helps predict how a system at equilibrium will respond to changes in concentration, temperature, or pressure.

Effect of Volume Change on Gaseous Equilibria

In gaseous equilibria, a decrease in volume increases the pressure of the system. According to Le Chatelier's Principle, the equilibrium will shift toward the side with fewer moles of gas to reduce the pressure. Conversely, an increase in volume decreases pressure, shifting the equilibrium toward the side with more moles of gas.

Stoichiometry of the Reaction

Understanding the stoichiometry of the reaction is crucial for predicting shifts in equilibrium. In the reaction CO(g) + H2O(g) ⇌ CO2(g) + H2(g), there are 2 moles of gas on the left and 2 moles on the right. Since the number of moles is equal, a volume change will not favor either side, leading to no effect on the equilibrium position.