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R\(\rightarrow\)P is a first order reaction. For this reaction a graph of ln[R] (on y-axis) and time (on x-axis) gave a straight line with negative slope. The intercept on y-axis is equal to (k=rate constant)

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Memorize the graphical representations of the integrated rate laws: - \textbf{Zero Order:} A plot of \([R]\) vs. time is linear with slope \(-k\). - \textbf{First Order:} A plot of \(\ln[R]\) vs. time is linear with slope \(-k\). - \textbf{Second Order:} A plot of \(1/[R]\) vs. time is linear with slope \(+k\).

Updated On: Mar 30, 2026

ln[R]\(_0\)
[R]\(_0\)
k \(\times\) 2.303
\( \frac{k}{2.303} \)

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The Correct Option is A

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