For a first order reaction graph is plotted between logR0R on Y-axis against time (t) on X-axis. Slope of the line is equal to[R0 = initial concentration of reactant;R= concentration of reactant at time t,and K = first order rate constant]

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For a first order reaction graph is plotted between $\log \frac{R_{0}}{R}$ on Y-axis against time (t) on

X-axis. Slope of the line is equal to[R₀ = initial concentration of reactant;R= concentration of reactant at time t,and K = first order rate constant]

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$\frac{K}{2.303}$

$- \frac{K}{2.303 t}$

$\frac{K}{2.303 t}$

$- \frac{K}{2.303}$

answer is B.

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Detailed Solution

$\log \frac{[R_{0}]}{[R]} = \frac{K}{2.303} \times t$

y = mx

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