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Given [A] = 0.01 M, Rate = 2.0 × 10⁻³ mol L⁻¹ s⁻¹. For a first order reaction, calculate the rate constant k.

1. k = 2.0 × 10⁻³ / [0.01] = 2 × 10⁻¹
2. k = 2.0 × 10⁻³ / [0.01] = 2 × 10⁻²
3. k = 2.0 × 10⁻³ / [0.01] = 2 × 10⁻³
4. k = 2.0 × 10⁻³ / [0.01] = 2 × 10⁻⁴

Correct answer: k = 2.0 × 10⁻³ / [0.01] = 2 × 10⁻²

Solution

For a first-order reaction, the rate law is Rate = k[A]. Rearranging, k = Rate / [A]. Substituting the given values, k = (2.0 × 10⁻³) / (0.01) = 2 × 10⁻¹. Thus, option B is correct.

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