The decomposition of N 2 O 5 (g) to NO 2 (g) and O 2 (g) obeys first-order kinetics. Assume the form of the rate law is Rate where k = 3.4 × 10 -5 s -1 at 25°C. -The reaction A → B + C is known to be zero order in A with a rate constant of 3.8× 10^-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 1.0 × 10^-3 M. What is the rate after 6.5 minutes?

Question

Quizplus · Accepted Answer

Since the reaction is zero order in A, the rate is solely dependent on the rate constant. Thus, rate = k[A] = (3.8×10^-2 mol/L*s) * (1.0×10^-3 M) = 3.8×10^-5 mol/L*s. This rate will remain constant over time as it is not affected by the concentration of A. Therefore, the rate after 6.5 minutes is still 3.8×10^-5 mol/L*s, or choice B.

The Decomposition of N2O5(g) to NO2(g) and O2(g) Obeys First-Order

The Decomposition of N₂O₅(g) to NO₂(g) and O₂(g) Obeys First-Order