. The rate constant for a first order reaction is $4.606 \times 10^{-3} \mathrm{~s}^{-1}$. The time required to reduce $2.0 \mathrm{~g}$ of the reactant to $0.2 \mathrm{~g}$ is :

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. The rate constant for a first order reaction is $4.606 \times 10^{-3} \mathrm{~s}^{-1}$. The time required to reduce $2.0 \mathrm{~g}$ of the reactant to $0.2 \mathrm{~g}$ is :

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deepak01 · Answer 1 · 2021-12-30T09:26:22+0000

Solution:
$$
\begin{aligned}
&K=\frac{2.303}{t} \log \frac{a}{a-x} \\
&t=\frac{2.303}{4.606 \times 10^{-3}} \\
&\log \frac{2}{0.2} \\
&=\frac{1000}{2} \log 10 \\
&=500 \mathrm{sec} \\
&\text { (as log } 10=1 \text { ) }
\end{aligned}
$$

. The rate constant for a first order reaction is \(4.606 \times 10^{-3} \mathrm{~s}^{-1}\). The time required to reduce \(2.0 \mathrm{~g}\) of the reactant to \(0.2 \mathrm{~g}\) is :

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