Textbook Question
What are the units of k for each type of reaction?
a. first-order reaction
b. second-order reaction
c. zero-order reaction
1049
views
Ch.15 - Chemical Kinetics
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 15, Problem 43c
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if the concentrations of all three reactants are doubled?
Verified step by step guidance1
Identify the rate law for the reaction. Since the reaction is first order in A, second order in B, and zero order in C, the rate law can be expressed as: \( \text{Rate} = k[A]^1[B]^2[C]^0 \).
Recognize that a zero order in C means that changes in the concentration of C do not affect the rate of the reaction.
Focus on the effect of doubling [A] while keeping [B] and [C] constant. Substitute the new concentration of A into the rate law: \( \text{New Rate} = k(2[A])^1[B]^2[C]^0 \).
Simplify the expression for the new rate: \( \text{New Rate} = 2k[A][B]^2 \).
Compare the new rate to the original rate: \( \text{New Rate} = 2 \times \text{Original Rate} \). Therefore, the reaction rate doubles when [A] is doubled.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Reaction Order
Reaction order refers to the power to which the concentration of a reactant is raised in the rate law of a chemical reaction. It indicates how the rate of reaction is affected by the concentration of that reactant. In this case, the reaction is first order in A, second order in B, and zero order in C, meaning that the rate depends linearly on [A], quadratically on [B], and is independent of [C].
Recommended video:
Guided course
00:36
Average Bond Order
Rate Law
The rate law expresses the relationship between the rate of a chemical reaction and the concentration of its reactants. It is typically written in the form Rate = k[A]^m[B]^n[C]^p, where k is the rate constant, and m, n, and p are the orders of the reaction with respect to each reactant. For the given reaction, the rate law can be expressed as Rate = k[A]^1[B]^2[C]^0, highlighting how changes in concentrations affect the overall reaction rate.
Recommended video:
Guided course
01:52Rate Law Fundamentals
Effect of Concentration Change on Reaction Rate
When the concentration of a reactant is changed, the reaction rate changes according to its order. For a first-order reactant, doubling the concentration will double the rate, while for a second-order reactant, it will quadruple the rate. In this scenario, since [A] is doubled and it is first order, the reaction rate will also double, while the concentrations of B and C remain constant.
Recommended video:
Guided course
02:10Concentration Changes and Rate Law Example
Related Practice
Textbook Question
A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?
2570
views
Textbook Question
A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. a. Write a rate law for the reaction.
833
views
Textbook Question
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C. b. What is the overall order of the reaction?
422
views
Textbook Question
Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k.
[A] (M) Initial Rate (M/s)
0.050 0.100
0.075 0.225
0.090 0.324
1
views
Textbook Question
This reaction is first order in N2O5: N2O5(g) → NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. a. Calculate the rate of the reaction when [N2O5] = 0.055 M
531
views