The reaction
2N₂O₅(g) → O₂(g) + 4NO₂(g)
Is first order in N₂O₅. For this reaction at 45° C, the rate constant k = 1.0 × 10^-5 s^-1, where the rate law is defined as
Rate
For a particular experiment ([N₂O₅]₀ = 1.0 × 10^-3 M) , calculate [N₂O₅] after 1.0 × 10⁵ s.

Question

The reaction
2N₂O₅(g) → O₂(g) + 4NO₂(g)
Is first order in N₂O₅. For this reaction at 45° C, the rate constant k = 1.0 × 10^-5 s^-1, where the rate law is defined as
Rate

The reaction 2N<sub>2</sub>O<sub>5</sub>(g) → O<sub>2</sub>(g) + 4NO<sub>2</sub>(g) Is first order in N<sub>2</sub>O<sub>5</sub>. For this reaction at 45° C, the rate constant k = 1.0 × 10<sup>-5</sup> s<sup>-1</sup>, where the rate law is defined as Rate For a particular experiment ([N<sub>2</sub>O<sub>5</sub>]<sub>0</sub> = 1.0 × 10<sup>-3</sup> M) , calculate [N<sub>2</sub>O<sub>5</sub>] after 1.0 × 10<sup>5</sup> s. A) 0 B) 5.0 × 10<sup>-4</sup> M C) 3.7 × 10<sup>-4</sup> M D) 1.0 × 10<sup>-3</sup> M E) none of these

For a particular experiment ([N₂O₅]₀ = 1.0 × 10^-3 M) , calculate [N₂O₅] after 1.0 × 10⁵ s.

Quizplus · Accepted Answer

Using the first-order rate law, we can determine the concentration of N₂O₅ remaining after a certain amount of time: ln(N₂O₅t/N₂O₅o) = -kt where t is time, o denotes the initial concentration, and k is the rate constant. Rearranging this equation gives: N₂O₅t = N₂O₅o * e^(-kt) Plugging in the given values, we get: N₂O₅t = (1.0 × 10^-3 M) * e^(-(1.0 × 10^-5 s^-1)(1.0 × 10^15 s)) N₂O₅t = 3.7 × 10^-4 M Therefore, the concentration of N₂O₅ remaining after 1.0 × 10^15 s is 3.7 × 10^-4 M, which is choice C.

The Reaction 2N2O5(g) → O2(g) + 4NO2(g)

The Reaction 2N₂O₅(g) → O₂(g) + 4NO₂(g)