Which of the following best explains the effects of a catalyst on the rate of a reversible reaction?
Correct answer: D. It provides a new reaction path with a lower activation energy.
- A. It decreases the rate of the reverse reaction.
- B. It increases the kinetic energy of the reacting molecules.
- C. It moves the equilibrium position to the right.
- D. It provides a new reaction path with a lower activation energy.
Explanation
A catalyst affects the rate of a reversible reaction by providing an alternative pathway with a lower activation energy, thereby increasing the rate at which equilibrium is reached. It does not change the equilibrium position or selectively affect the forward or reverse reaction rates differently. Option D is correct because it accurately describes the role of a catalyst in reaction kinetics. Option A is incorrect because a catalyst speeds up both forward and reverse reactions equally, not just one. Option B is incorrect because a catalyst does not change the kinetic energy of the reacting molecules. Option C is incorrect because the equilibrium position remains unchanged by a catalyst; it only affects the rate of reaching equilibrium.
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About Reaction Kinetics
Reaction kinetics relates reaction rate to concentration, temperature, surface area and catalysts. Questions cover rate laws, reaction order, rate constants, activation energy and the activated complex, including how a catalyst lowers the activation energy without changing the overall energy change or equilibrium position.
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