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For a first order reaction $A\rightarrow$ Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in $min^{-1}$ is
A
0.2303
B
1.3818
C
0.9212
D
0.4606
Detailed Solution
For a first order reaction: $k = \frac{2.303}{t}\log\frac{[A]_0}{[A]_t}$
$k = \frac{2.303}{5}\log\frac{0.1}{0.001} = \frac{2.303}{5} \times 2$
$k = 0.9212\ min^{-1}$