Catalysts Reduce Activation Energy in Reactions

Steps:

• Define activation energy as the minimum energy barrier for reactants to form products.
• Recall that reaction rate depends on factors like collision frequency and activation energy.
• Evaluate each option: only catalysts directly alter the energy pathway.
• Confirm that lowering activation energy speeds up the reaction without changing other conditions.

Why A is correct:

• Catalysts provide an alternative reaction pathway with lower activation energy, increasing the rate constant per the Arrhenius equation (k = A e^(-Ea/RT)).

Why the others are wrong:

• B: Increases surface area boosts collision frequency between particles, not activation energy.
• C: Raises acid concentration increases reactant collisions, without affecting activation energy.
• D: Elevates temperature gives particles more kinetic energy to surpass the activation energy barrier, but does not lower it.

Final answer: A