A) \[k=\frac{2.303}{t}\log \,\left( \frac{{{A}_{0}}}{{{A}_{t}}} \right)\]
B) \[k=\frac{t}{2.303}\log \,\left( \frac{{{A}_{0}}}{{{A}_{t}}} \right)\]
C) \[-k=\frac{t}{2.303}\log \,\left( \frac{{{A}_{t}}}{{{A}_{0}}} \right)\]
D) Rate \[=k[A]\]
Correct Answer: B
Solution :
The rate of first order reaction is expressed as A \[\xrightarrow{{}}\] Products Rate \[=\frac{d[A]}{dt}\] Rate \[=k[A]\] and the rate constant (k) is expressed as \[k=\frac{2.303}{t}\log \frac{[{{A}_{0}}]}{[{{A}_{t}}]}\] \[k=\frac{t}{2.303}\log \frac{[{{A}_{t}}]}{[{{A}_{o}}]}\]
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