Answer:
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Explanation:
A <em>first order reaction</em> follows the law:
, where [A] is the concentraion of the reactant A.
Equivalently:
![\dfrac{d[A]}{dt}=-k[A]](https://tex.z-dn.net/?f=%5Cdfrac%7Bd%5BA%5D%7D%7Bdt%7D%3D-k%5BA%5D)
Integrating:
![\dfrac{d[A]}{[A]}=-kdt](https://tex.z-dn.net/?f=%5Cdfrac%7Bd%5BA%5D%7D%7B%5BA%5D%7D%3D-kdt)
![\ln \dfrac{[A]}{[A_o]}=-kt](https://tex.z-dn.net/?f=%5Cln%20%5Cdfrac%7B%5BA%5D%7D%7B%5BA_o%5D%7D%3D-kt)
Half-life means [A]/[A₀] = 1/2, t = t½:
That means that the half-life is constant.
The slope of the plot of ln [N₂O₅] is -k. Then k is equal to 6.40 × 10⁻⁴ min⁻¹.
Thus, you can calculate t½:
t½ = ln(2) / 6.40 × 10⁻⁴ min⁻¹
t½ = 1,083 min.
Rounding to 3 significant figures, that is 1,080 min.