Which of the following best describes the common strategy by which catalysis occurs in chemical reactions?

• A. Catalysts raise the $\mathrm{activation energy}$ to slow down the reaction.
• B. Catalysts are consumed during the reaction and become part of the final products.
• C. Catalysts provide an alternative reaction pathway with a lower $\mathrm{activation energy}$.
• D. Catalysts increase the $\mathrm{equilibrium constant}$ of the reaction.

Answer: (C)

Verified step by step guidance

1. Understand that catalysis involves the use of a catalyst to speed up a chemical reaction without being consumed in the process.
2. Recall that the activation energy (\[E_a\]) is the energy barrier that must be overcome for reactants to convert into products.
3. Recognize that catalysts work by providing an alternative reaction pathway that has a lower activation energy compared to the uncatalyzed reaction.
4. Note that lowering the activation energy increases the rate at which equilibrium is reached but does not change the equilibrium constant (\[K_{eq}\]) of the reaction.
5. Conclude that the correct description of catalysis is that catalysts provide an alternative reaction pathway with a lower activation energy, thereby increasing the reaction rate without being consumed or altering the equilibrium position.