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The rate constant for a first order reaction is $4.606\times10^{-3}\ s^{-1}$. The time required to reduce 2.0 g of the reactant to 0.2 g is:
A
200 s
B
500 s
C
1000 s
D
100 s
Detailed Solution
For a first order reaction: $k = \frac{2.303}{t}\log\frac{A_0}{A}$
$4.606 \times 10^{-3} = \frac{2.303}{t}\log\frac{2}{0.2}$
$t = \frac{2.303}{4.606 \times 10^{-3}} \times \log 10 = \frac{10^3}{2} = 500$ s