Which statement is true about activation energy in catalyzed reactions?

Which statement is true about activation energy in catalyzed reactions?

• A. Catalysts provide an alternate pathway with lower activation energy
• B. Catalysts increase the activation energy
• C. Catalysts require higher temperatures to be effective
• D. Catalysts double the activation energy

Answer: (A)

Activation energy is the energy barrier that must be overcome for a reaction to proceed. A catalyst provides an alternate reaction pathway with a lower energy barrier by stabilizing the transition state or forming temporary intermediates. With a smaller barrier, more molecules have enough energy at a given temperature to react, so the rate increases without changing the overall energy difference between reactants and products. Catalysts do not change ΔG or the equilibrium position, and they do not require higher temperatures to work; in fact, they often allow the reaction to run efficiently at lower temperatures. They also do not raise or double the activation energy, which would slow the process.

Activation energy is the energy barrier that must be overcome for a reaction to proceed. A catalyst provides an alternate reaction pathway with a lower energy barrier by stabilizing the transition state or forming temporary intermediates. With a smaller barrier, more molecules have enough energy at a given temperature to react, so the rate increases without changing the overall energy difference between reactants and products. Catalysts do not change ΔG or the equilibrium position, and they do not require higher temperatures to work; in fact, they often allow the reaction to run efficiently at lower temperatures. They also do not raise or double the activation energy, which would slow the process.