Coal can be used to generate hydrogen gas (a potential fuel) by the endothermic reaction: C(s) + H₂O(g) ⇌ CO(g) + H₂(g) If this reaction mixture is at equilibrium, predict whether each disturbance will result in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. e. adding a catalyst to the reaction mixture

Key Concepts

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this state, any changes to the system, such as concentration, pressure, or temperature, can shift the equilibrium position according to Le Chatelier's principle, which predicts how the system will respond to disturbances.

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. For example, if the concentration of a reactant is increased, the system will shift to favor the formation of products, thereby increasing the amount of hydrogen gas in this reaction.

Catalysts and Reaction Rates

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. While catalysts lower the activation energy required for a reaction, they do not affect the position of equilibrium; thus, adding a catalyst to the reaction mixture will speed up the attainment of equilibrium but will not change the amounts of hydrogen gas produced at equilibrium.