For the following equilibria, use Le Châtelier's principle to predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture. C(s) + H2O(g) ⇌ CO(g) + H2(g)

Le Châtelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract that change and restore a new equilibrium. This principle is crucial for predicting how a system at equilibrium responds to changes in concentration, temperature, or pressure.

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. The reaction quotient (Q) helps determine the direction in which the reaction will shift to reach equilibrium, based on the concentrations of the reactants and products at any given moment.

In gaseous reactions, changes in pressure affect the equilibrium position based on the number of moles of gas on each side of the reaction. According to Le Châtelier's Principle, increasing pressure by decreasing volume will favor the side of the reaction with fewer moles of gas, thus shifting the equilibrium to minimize the pressure change.