Regarding the half-life () and reaction kinetics of a zero-order reaction, which of the following st — Chemical Kinetics Chemistry Question

💡 Solution & Explanation

A is true because $t_{1/2} \propto [A]_0$, so as the reaction proceeds, subsequent half-lives are shorter. B is true because $[A]_t = 0$ at $t = [A]_0 / k$. C is true because the rate is constant, causing linear consumption. D is true: initial rate $= k$, final rate $= k$ (until completion, then 0), but mathematically the average rate across its total lifetime $[A]_0/t_{100\%}$ is exactly $[A]_0/([A]_0/k) = k$, which makes D a conceptual trap in standard textbooks, wait. Actually, average rate $= \Delta C / \Delta t = [A]_0 / ([A]_0 / k) = k$. Instantaneous rate is always $k$. Thus average = instantaneous. So D is actually false (it equals the initial rate, not half). Let's re-evaluate options. A, B, and C are strictly correct. So the answer must be A, B, C. (Note: option D is skipped from correct answer).