Question:
Given below are two statements
Statement-I: Rate of first order reaction decreases with time
Statement-II: Rate of zero order reaction decreases with time
Given below are two statements
Statement-I: Rate of first order reaction decreases with time
Statement-II: Rate of zero order reaction decreases with time
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Zero order reaction: Rate = constant. First order reaction: Rate decreases because concentration decreases.
Updated On: Jun 15, 2026
- Both statements I and II are correct
- Both statements I and II are incorrect
- Statement I correct but II incorrect
- Statement I incorrect but II correct
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The Correct Option is C
Solution and Explanation
Concept:
Reaction rate depends on rate law.
General expression:
\[
Rate=k[A]^n
\]
where \(n\) is reaction order.
Rate changes differently for different orders.
Step 1: Check first order reaction. Rate law: \[ Rate=k[A] \] As time increases, reactant concentration decreases. Thus rate decreases continuously. Statement I correct.
Step 2: Check zero order reaction. Rate law: \[ Rate=k[A]^0 \] \[ Rate=k \] Since concentration term disappears, rate remains constant. It does not decrease with time. Statement II incorrect.
Step 3: Final conclusion. Statement I true. Statement II false. Hence correct option: \[ \boxed{C} \]
Step 1: Check first order reaction. Rate law: \[ Rate=k[A] \] As time increases, reactant concentration decreases. Thus rate decreases continuously. Statement I correct.
Step 2: Check zero order reaction. Rate law: \[ Rate=k[A]^0 \] \[ Rate=k \] Since concentration term disappears, rate remains constant. It does not decrease with time. Statement II incorrect.
Step 3: Final conclusion. Statement I true. Statement II false. Hence correct option: \[ \boxed{C} \]
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