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 :

Engineering

Chemistry

Integrated Rate Law

Question

3.47 × 10^–4 M/min

1.73 × 10^–5 M/min

3.47 × 10^–5 M/min

1.73 × 10^–4 M/min

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$0 .1 M \overset{t_{1 / 2}}{\to} 0 .05 M \to_{}^{t_{1 / 2}} 0 .025 M$

$∴$ t_1/2 = 40/2 = 20 min

Now, r = K [A] = $\frac{0.693}{20 \min} \times 0.01$

= 3.47 × 10^–4 M/ min Ans.