The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 2.88 M,what is the concentration of N₂O₅ after 12.5 minutes?

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Quizplus · Accepted Answer

The concentration after a given time in a first-order reaction is calculated using the formula $[A]_t = [A]_0 e^{-kt}$, where $[A]_t$ is the concentration at time $t$, $[A]_0$ is the initial concentration, $k$ is the rate constant, and $t$ is the time in seconds. Given $k = 1.70 \times 10^{-3} \, \text{s}^{-1}$, $[A]_0 = 2.88 \, \text{M}$, and $t = 12.5 \, \text{minutes} = 750 \, \text{seconds}$, substituting these values into the formula gives a concentration of approximately $0.805 \, \text{M}$.

The First-Order Decomposition of N2O5 at 328 K Has a Rate

The First-Order Decomposition of N₂O₅ at 328 K Has a Rate