Skip to main content
Pearson+ LogoPearson+ Logo
Ch.14 - Chemical Kinetics
All textbooksBrown 14th EditionCh.14 - Chemical KineticsProblem 91b
Previous problem
Next problem
Chapter 14, Problem 91b

The reaction 2 NO(g) + O2(g) → 2 NO2 (g) is second order in NO and first order in O2. When [NO] = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10-5 M/s. (b) What is the value of the rate constant?

Verified Solution

Video duration:
2m
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Rate Law

The rate law expresses the relationship between the rate of a chemical reaction and the concentration of its reactants. For the given reaction, the rate law can be written as Rate = k[NO]^2[O2]^1, where k is the rate constant. Understanding the rate law is essential for determining how changes in concentration affect the reaction rate.
Recommended video:
Guided course
01:52
Rate Law Fundamentals

Order of Reaction

The order of a reaction refers to the power to which the concentration of a reactant is raised in the rate law. In this case, the reaction is second order with respect to NO and first order with respect to O2. The overall order of the reaction is the sum of the individual orders, which helps in calculating the rate constant and understanding the kinetics of the reaction.
Recommended video:
Guided course
00:36
Average Bond Order

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law that is specific to a given reaction at a certain temperature. It reflects the speed of the reaction and can be determined using the observed rate and concentrations of the reactants. Calculating k is crucial for predicting how the reaction will behave under different conditions.
Recommended video:
Guided course
01:14
Equilibrium Constant K
Previous problem
Next problem
Related Practice
Textbook Question

The activation energy of an uncatalyzed reaction is 95 kJ/mol. The addition of a catalyst lowers the activation energy to 55 kJ/mol. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (b) 125 °C?

1218
views
Textbook Question

Consider the reaction A + B → C + D. Is each of the following statements true or false? (b) If the reaction is an elementary reaction, the rate law is second order.

373
views
Textbook Question

Consider the reaction A + B → C + D. Is each of the following statements true or false? (c) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order.

775
views
Textbook Question

The reaction 2 NO(g) + O2(g) → 2 NO2 (g) is second order in NO and first order in O2. When [NO] = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10-5 M/s. (c) What are the units of the rate constant?

735
views
Textbook Question

Consider the following reaction between mercury(II) chloride and oxalate ion: 2 HgCl21aq2 + C2O4 2 - 1aq2¡2 Cl - 1aq2 + 2 CO21g2 + Hg2Cl21s2 The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O4 2 -, and the following rate data were obtained for the rate of disappearance of C2O4 2 - : Experiment 3HgCl2 4 1M 2 3C2o4 24 1M 2 Rate 1M,s2 1 0.164 0.15 3.2 * 10-5 2 0.164 0.45 2.9 * 10-4 3 0.082 0.45 1.4 * 10-4 4 0.246 0.15 4.8 * 10-5 (c) What is the reaction rate when the initial concentration of HgCl2 is 0.100 M and that of C2O4 2- is 0.25 M if the temperature is the same as that used to obtain the data shown?

1289
views
Textbook Question

The reaction 2 NO2¡2 NO + O2 has the rate constant k = 0.63 M- 1s - 1. (b) If the initial concentration of NO2 is 0.100 M, how would you determine how long it would take for the concentration to decrease to 0.025 M?

1325
views