How do catalysts increase the rate of a chemical reaction?

• A. By lowering the activation energy required for the reaction to occur
• B. By increasing the equilibrium constant of the reaction
• C. By providing additional energy to the reactants
• D. By increasing the concentration of reactants

Answer: (A)

Verified step by step guidance

1. Understand that the rate of a chemical reaction depends on how quickly reactants are converted into products, which is influenced by the activation energy (Ea) — the minimum energy needed for the reaction to proceed.
2. Recognize that catalysts work by providing an alternative reaction pathway with a lower activation energy, making it easier for reactant molecules to reach the transition state.
3. Note that lowering the activation energy increases the number of reactant molecules that have enough energy to react at a given temperature, thus increasing the reaction rate.
4. Clarify that catalysts do not change the equilibrium constant of the reaction; they only help the system reach equilibrium faster by speeding up both the forward and reverse reactions equally.
5. Understand that catalysts do not provide additional energy to reactants nor do they change reactant concentrations; their role is solely to lower the activation energy barrier.