The incorrect statement is: “Catalysts increase the amount of product made.” Catalysts speed up the reaction by lowering activation energy, but they do not change the equilibrium yield or final amount of product.

Why this is incorrect

  • A catalyst increases the rate of reaction, not the equilibrium position.
  • It can be recovered after the reaction and is not permanently consumed.
  • It works by providing an alternative pathway with lower activation energy.

In simple terms

A catalyst helps the reaction happen faster, but it does not create extra product beyond what the reactants can ultimately form.

If you share the answer choices, I can identify the exact option letter.