For the first-order reaction A → products, what is the reaction rate when [A] = 0.201 M and k = 0.360 min^{-1}?

• A. 0.0724 M/min
• B. 0.360 M/min
• C. 0.201 M/min
• D. 0.561 M/min

Answer: (A)

Verified step by step guidance

1. Identify the order of the reaction and the given data. Here, the reaction is first-order with respect to A, the concentration [A] = 0.201 M, and the rate constant k = 0.360 min^{-1}.
2. Recall the rate law for a first-order reaction, which is given by the equation: \(\text{rate} = k \times [A]\).
3. Substitute the given values into the rate law: \(\text{rate} = 0.360\ \text{min}^{-1} \times 0.201\ \text{M}\).
4. Multiply the rate constant by the concentration to find the reaction rate in units of M/min.
5. Express the final rate with the correct units and compare it to the provided answer choices to select the correct one.