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The reaction $X \to products$ follows first order kinetics in 40 minutes the concentration of x change from 0.1 M to 0.025 M. The rate of reaction when concentration of x is 0.01 M

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$1.37 \times 10^{- 4} M \min^{- 1}$

$3.47 \times 10^{- 5} M \min^{- 1}$

$3.47 \times 10^{- 4} M \min^{- 1}$

$1.73 \times 10^{- 5} M \min^{- 1}$

answer is C.

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Detailed Solution

$k = \frac{2.303}{t} \log \frac{{[A]}_{0}}{[A]} k = \frac{2.303}{40} \log \frac{0.1}{0.025}$

$= 0.0347 \min^{- 1}$

$Rate = k [A] Rate = 0.0347 \times 10^{- 2} M \min^{- 1} Rate = 3.47 \times 10^{- 4} mol L^{- 1} \min^{- 1}$

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