The time for the half-life period of a certain zero-order reaction is . When the initial concentrati — Chemical Kinetics Chemistry Question
Question
The time for the half-life period of a certain zero-order reaction $A \rightarrow \text{Products}$ is $1 \text{ hour}$. When the initial concentration of reactant $A$ is $2.0 \text{ mol L}^{-1}$, how much time in hours does it take for its concentration to drop from $0.50 \text{ M}$ to $0.25 \text{ M}$?
Answer: 0.25
💡 Solution & Explanation
For zero order, $t_{1/2} = [A]_0 / 2k$. Given $[A]_0 = 2.0 \text{ M}$ and $t_{1/2} = 1 \text{ h}$, $1 = 2.0 / 2k \Rightarrow k = 1.0 \text{ M h}^{-1}$. The time to go from $0.50 \text{ M}$ to $0.25 \text{ M}$ is $\Delta t = \Delta [A] / k = (0.50 - 0.25) / 1.0 = 0.25 \text{ hours}$.
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