Question:

Which of the following equation exhibits integrated rate law equation for first order reaction?

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First order key form: $k = \frac{2.303}{t} \log \frac{a}{a-x}$
Updated On: May 8, 2026
  • $\text{k} = \frac{[\text{A}]_0 - [\text{A}]_t}{t}$
  • $\text{k} = \frac{2.303}{t} \times \log \frac{\text{a}}{(\text{a}-\text{x})}$
  • $k = \frac{1}{t} \ln \frac{(\text{a}-\text{x})}{\text{a}}$
  • $\text{k} = \frac{1}{\text{t}} \times \frac{\text{x}}{\text{a}(\text{a}-\text{x})}$
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The Correct Option is B

Solution and Explanation


Concept: Integrated rate law for first order reaction: \[ k = \frac{2.303}{t} \log \frac{a}{a-x} \] or \[ k = \frac{1}{t} \ln \frac{a}{a-x} \]

Step 1:
Compare options.
• (A) Zero order equation
• (B) Correct first order equation
• (C) Incorrect (log form reversed)
• (D) Second order equation

Step 2:
Conclusion.
Thus, correct equation is option (B). Final Answer: Option (B)
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