MP Board · Class 12 · Chemistry · Chemical KineticsFor a first-order reaction, the time required for 99.9% completion is approximately equal to:
📊Student Analytics & Stats
Total Attempts: 5
Accuracy Rate: 20%
Step-by-Step Solution
Using $t = \frac{2.303}{k} \log \frac{[A]_0}{[A]}$, for 99.9% completion, $[A] = [A]_0 - 0.999[A]_0 = 0.001[A]0$. Thus, $t = \frac{2.303}{k} \log(1000) = \frac{2.303 \times 3}{k} = \frac{6.93}{k} = 10 \times t{1/2}$.
Detailed Options Breakdown
Option : 2 times half-life
Incorrect choice. This distractor represents a common misunderstanding of the core principles of Chemical Kinetics.
Option 1: 5 times half-life
Incorrect choice. This distractor represents a common misunderstanding of the core principles of Chemical Kinetics.
Option 2: 10 times half-life (Correct Answer)
Correct choice. Refer to the step-by-step verified solution guidelines above for details.
Option 3: 100 times half-life
Incorrect choice. This distractor represents a common misunderstanding of the core principles of Chemical Kinetics.
💡 Study Guide: This question tests core syllabus concepts from Chemical Kinetics. For formulas, key summaries, and mock exam reference guides, read the full Chemical Kinetics Revision Notes.