Exhibit 13-14 Consider the decomposition of N₂O₅ as shown in the equation below to answer the following question(s) . 2 N₂O₅ (g) →4 NO₂ (g) + O₂ (g) This reaction has been determined to be first order with respect to N₂O₅.
-Refer to Exhibit 13-14. If 0.0250 moles of N₂O₅ are charged into a 2.00 L vessel, how many moles will remain after 150 seconds if the rate constant is 6.82×10^{- 3} s^{- 1} (at 70 ° C) ?

Question

Quizplus · Accepted Answer

The first-order reaction formula is used: [A] = [A]₀e^(-kt). Initial concentration [A]₀ = 0.0250 moles / 2.00 L = 0.0125 M. After 150 seconds, [A] = 0.0125 * e^(-6.82×10^-3 * 150) = 0.004495 M. Multiply by volume (2.00 L) to get moles: 0.004495 * 2.00 = 8.99×10^-3 moles.

Exhibit 13-14 Consider the Decomposition of N2O5 as Shown in the Equation

Exhibit 13-14 Consider the Decomposition of N₂O₅ as Shown in the Equation