Catalysts accelerate reactions by lowering activation energy

Steps:

• Recall that catalysts provide an alternative pathway with lower activation energy, increasing reaction rate without shifting equilibrium.
• Evaluate statement 1: Catalysts do not alter the equilibrium position, as they speed up both forward and reverse reactions equally.
• Evaluate statement 2: Catalysts decrease activation energy, enabling more molecules to react at a given temperature.
• Evaluate statement 3: Catalysts increase the reaction rate by facilitating more frequent successful collisions.

Why C is correct:

• Option C selects statements 2 and 3, which align with the definition of catalysts lowering activation energy (E_a) and increasing rate constant (k) per the Arrhenius equation: k = A e^(-E_a/RT).

Why the others are wrong:

• A includes incorrect statement 1, as catalysts do not change equilibrium.
• B pairs wrong statement 1 with correct 3, omitting valid 2.
• D ignores correct statements 2 and 3, selecting only 3.

Final answer: C