The half life period of a first order chemical reaction is $6.93$ minutes. The time required for the completion of $99 \%$ of the chemical reaction will be $(\log 2=0.301)$ :

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Aicharya · Accepted Answer

$ \begin{aligned} & \because \lambda=\frac{0.6932}{t_{1 / 2}}=\frac{0.6932}{6.93} \min ^{-1} \ & 	ext { Also } t=\frac{2.303}{\lambda} \log \frac{\left[A_{\circ}ight]}{[A]} \ & {\left[A_{\circ}ight]=	ext { initial concentration (amount) }} \ & {[A]=	ext { final concentration (amount) }} \ & 	herefore t=\frac{2.303 	imes 6.93}{0.6932} \log \frac{100}{1} \ & =46.06 	ext { minutes } \end{aligned} $

The half life period of a first order chemical reaction is $6.93$ minutes. The time required for the…

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