The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1.If the initial concentration of N₂O is 10.9 M,what is the concentration of N₂O after 9.6 s?

Question

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The integrated rate law for a first-order reaction is:ln[A]t = -kt + ln[A]0where [A]t is the concentration of the reactant at time t, k is the rate constant, and [A]0 is the initial concentration of the reactant.We can use this equation to solve for the concentration of N2O after 9.6 s:ln[N2O]t = -0.76 s-1 * 9.6 s + ln(10.9 M)ln[N2O]t = -7.344[N2O]t = e-7.344 = 7.4 × 10-3 MTherefore, the concentration of N2O after 9.6 s is 7.4 × 10-3 M.

The First-Order Decomposition of N2O at 1000 K Has a Rate

The First-Order Decomposition of N₂O at 1000 K Has a Rate