For the reaction 2N2O5(g) → 4NO2(g) + O2(g) with a rate constant k = 2.8×10⁻³ sec⁻¹, if the initial concentration of [N2O5] is 1.58 mol/L, what is the concentration of N2O5 after 300 seconds?

This reaction was monitored as a function of time: AB → A + B A plot of 1/[AB] versus time yields a straight line with a slope of +0.55/Ms.

d. If the initial concentration of AB is 0.250 M, and the reaction mixture initially contains no products, what are the concentrations of A and B after 75 s?

Consider the data presented in Exercise 14.19. (a) By using appropriate graphs, determine whether the reaction is first order or second order.

(b) How can you calculate the rate constant for a first-order reaction from the graph you made in part (a)?

As described in Exercise 14.41, the decomposition of sulfuryl chloride (SO₂Cl₂) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 × 10^-2 s^-1. (a) If we begin with an initial SO₂Cl₂ pressure of 450 torr, what is the partial pressure of this substance after 60 s?