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For the given first order reaction
\mathrm{A} \rightarrow \mathrm{B}
the half life of the reaction is 0.3010 \mathrm{~min}. The ratio of the initial concentration of reactant to the concentration of reactant at time 2.0 \mathrm{~min} will be equal to ______________.(Nearest integer)

Option: 1

100


Option: 2

-


Option: 3

-


Option: 4

-


Answers (1)

best_answer

Half Life = 0.3010 min

\mathrm{A\longrightarrow B}

From first order Reaction -
\mathrm{A= Ao\, e{-kt }\Rightarrow\, ln\, A= ln\, Ao\, -kt}
\mathrm{K= \frac{2.303}{t}\, log\frac{[Ao]}{[At]}\quad \quad t_{\frac{1}{2}}= \frac{k}{0.6} \; \frac{0.693}{k}}

\mathrm{\Rightarrow \frac{0.693}{t_{\frac{1}{2}}}= \frac{2.303}{2}\, log\left ( \frac{Ao}{At} \right )}             

\mathrm{log\, \frac{Ao}{At}= 2}
\mathrm{\therefore \frac{Ao}{At}= 10^{2}= 100}

Answer is 100

Posted by

vinayak

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