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(B) For a first order reaction,the time $t$ is given by: $t = \frac{2.303}{k} \log \frac{[A]_0}{[A]_t}$ Given: $k = 2.011 	imes 10^{-3} \ s^{-1}$ $[A

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$623$

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(B) For a first order reaction,the time $t$ is given by: $t = \frac{2.303}{k} \log \frac{[A]_0}{[A]_t}$ Given: $k = 2.011 	imes 10^{-3} \ s^{-1}$ $[A]_0 = 7 \ g$ $[A]_t = 2 \ g$ $\log 7 = 0.845$ $\log 2 = 0.301$ Substituting the values: $t = \frac{2.303}{2.011 	imes 10^{-3}} \log \left( \frac{7}{2} ight)$ $t = \frac{2.303}{2.011 	imes 10^{-3}} (\log 7 - \log 2)$ $t = \frac{2.303}{2.011 	imes 10^{-3}} (0.845 - 0.301)$ $t = \frac{2.303 	imes 0.544}{2.011} 	imes 10^3$ $t = \frac{1.252832}{2.011} 	imes 1000$ $t \approx 622.989 \ s$ The nearest integer is $623$.

If compound $A$ reacts with $B$ following first order kinetics with rate constant $2.011 \times 10^{-3} \ s^{-1}$. The time taken by $A$ (in seconds) to reduce from $7 \ g$ to $2 \ g$ will be $.........$ (Nearest Integer) $[\log 5=0.698, \log 7=0.845, \log 2=0.301]$

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