Which of the following statements is correct for the first-order reaction: A → 2B?

Question

Quizplus · Accepted Answer

For a first-order reaction, the rate of reaction is proportional to the concentration of the reactant. Therefore, the natural logarithm of the concentration of A follows a linear decrease with respect to time. This is represented by the equation ln[A] = -kt + ln[A]0, where [A]0 is the initial concentration of A and k is the rate constant. Choice A is incorrect because the concentration of A decreases exponentially, not linearly. Choice B is incorrect because the concentration of A decreases over time. Choice D is incorrect because the rate of reaction decreases over time as the concentration of A decreases. Choice E is incorrect because the rate constant does not change with respect to time for a first-order reaction.

Which of the Following Statements Is Correct for the First-Order