Question

Characteristics of second-order reactions

For a second-order reaction, [A]?products, the rate of the reaction is given as rate= k[A]2, where k is the rate constant and [A] is the concentration of reactant A. The integrated rate law for second-order reactions is 1[A]t=kt+1[A]0, where [A]t is the concentration of reactant A at time t, k is the rate constant, and [A]0 is the initial concentration of reactant A. This equation is of the type y=mx+b. Therefore, the plot of 1[A]t versus time is always a straight line with a slope k and a y intercept 1[A]0.

Part B

Consider the second-order reaction:

2NO2(g)?2NO(g)+O2(g)

Use the simulation to find the initial concentration [NO2]0 and the rate constant k for the reaction. What will be the concentration of NO2 after t = 40.0s ([NO2]t) for a reaction starting under the condition in the simulation?

Express your answer in moles per liters to three significant figures.

Characteristics of second-order reactions For a second-order reaction, [A]?products, the rate of the reaction is given as rate= k[A]2, where k is the rate constant and [A] is the concentration of reactant A. The integrated rate law for second-order reactions is 1[A]t=kt+1[A]0, where [A]t is the concentration of reactant A at time t, k is the rate constant, and [A]0 is the initial concentration of reactant A. This equation is of the type y=mx+b. Therefore, the plot of 1[A]t versus time is always a straight line with a slope k and a y intercept 1[A]0. Consider the second-order reaction: 2NO2(g)?2NO(g)+O2(g) Use the simulation to find the initial concentration [NO2]0 and the rate constant k for the reaction. What will be the concentration of NO2 after t = 40.0s ([NO2]t) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures.