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 concentra - Chemistry MCQ AIEEE 2012 2026 | ExamTest.live

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For a first order reaction, A \to 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:

Solution & Step-by-step Explanation

For a first order reaction: k = \frac{2.303}{t} lo g \frac{[ A ] _{0}}{[ A ]} k = \frac{2.303}{40} lo g \frac{0.1}{0.025} = \frac{2.303}{40} lo g 4 k = \frac{2.303}{40} \times 0.6020 \approx 0.03465 min^{- 1} Alternatively, 0.1 \to 0.05 \to 0.025 is two half-lives. 2 t_{1/2} = 40 ⟹ t_{1/2} = 20 min . k = \frac{0.693}{20} = 0.03465 min^{- 1} .Rate = k [A] : Rate = 0.03465 \times 0.01 = 3.465 \times 1 0^{- 4} M/min Rounding off, 3.47 \times 1 0^{- 4} M/min .

Try it yourself before checking the explanation above.

For a first order reaction, A \to 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:

1.73 \times 1 0^{- 5} M/min

3.47 \times 1 0^{- 4} M/min

3.47 \times 1 0^{- 5} M/min

1.73 \times 1 0^{- 4} M/min

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