Question

Which of the following represents the rate equation for a zero-order reaction?

• A. \( \text{Rate} = k[A] \)
• B. \( \text{Rate} = k[A]^2 \)
• C. \( \text{Rate} = k \)
• D. \( \text{Rate} = k[A]^n \)

Hint:

In a zero-order reaction, the rate does not depend on the concentration of the reactant.

Answer 1

The Correct Option is C

In a zero-order reaction, the rate of reaction is independent of the concentration of the reactants. The rate law for a zero-order reaction is simply: \[ \text{Rate} = k \] where \( k \) is the rate constant. This means that no matter how much of the reactant is present, the rate of the reaction remains constant over time. For the other options:
- Option (1) represents a first-order reaction.
- Option (2) represents a second-order reaction.
- Option (4) represents a general order reaction, where \( n \) can be any value.
Therefore, the correct answer is \( \text{Rate} = k \), representing a zero-order reaction.