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

Question

Quizplus · Accepted Answer

For a first-order reaction, the natural logarithm of the concentration of A is expected to decrease linearly with respect to time, according to the following equation: ln[A]t = -kt + ln[A]0. This is known as the integrated rate law for the first-order reaction. Option A is not correct because the concentration of A decreases exponentially, not linearly, with time. Option B is also not correct because the concentration of A changes with time. Option D is partially correct, but the rate of reaction decreases with time rather than being constant. Option E is not correct because the rate constant may be constant or change with time depending on the specific reaction conditions.

Which of the Following Statements Is Correct for the First-Order →\to→

Which of the Following Statements Is Correct for the First-Order $\to$