Question

Given below are two statements: 




In light of the above statements, choose the correct answer from the options given below:

• A. Statement I is false but Statement II is true
• B. Statement I is true but Statement II is false
• C. Both Statement I and Statement II are true
• D. Both Statement I and Statement II are false

Hint:

For first order reactions, the half-life is constant and independent of the initial concentration. Additionally, plotting \( \log [R] \) vs time gives a straight line with a slope related to the rate constant \( k \).

Answer 1

The Correct Option is B

- Statement (I) is false: The half-life (\( t_{1/2} \)) of a first-order reaction is independent of the initial concentration (\( [R_0] \)). The provided relationship between \( t_{1/2} \) and \( [R_0] \) is therefore incorrect.- Statement (II) is true: The integrated rate law for a first-order reaction is given by:\[\log [R] = \log [R_0] - \frac{k}{2.303} \cdot t.\]Plotting \( \log [R] \) against time yields a straight line with a slope equal to \( -\frac{k}{2.303} \). Final Answer: Statement I is false but Statement II is true.