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For a first order reaction, A → products, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is :

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$1.73 \times 10^{- 5} M / \min$

$3.47 \times 10^{- 4} M / \min$

$3.47 \times 10^{- 6} M / \min$

$1.73 \times 10^{- 4} M / \min$

answer is B.

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Detailed Solution

$\begin{array}{l} k = \frac{2.303}{40} \log \frac{0.1}{0.025} \\ k = \frac{0.693}{20} \end{array}$
$For a F . O . R ., rate = k [A]; rate = \frac{0.693}{20} \times 10^{- 2} = 3.47 \times 10^{- 4} M / \min .$

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