Textbook Question
This graph shows a plot of the rate of a reaction versus the concentration of the reactant.
a. What is the order of the reaction with respect to A?
Ch.15 - Chemical Kinetics
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Chapter 15, Problem 39b
What are the units of k for each type of reaction?
a. first-order reaction
b. second-order reaction
c. zero-order reaction
Verified step by step guidance1
Identify the type of reaction: In this case, it's a second-order reaction.
Understand the rate law for a second-order reaction: The rate law for a second-order reaction can be expressed as \(rate = k[A]^2\) or \(rate = k[A][B]\), where [A] and [B] are the concentrations of the reactants.
Analyze the units of rate and concentration: The rate of reaction is typically measured in \(\text{mol L}^{-1} \text{s}^{-1}\), and concentration is measured in \(\text{mol L}^{-1}\).
Set up the equation to find the units of k: Using the rate law, substitute the units into the equation. For example, if the rate law is \(rate = k[A]^2\), then substituting the units gives \(\text{mol L}^{-1} \text{s}^{-1} = k(\text{mol L}^{-1})^2\).
Solve for the units of k: Rearrange the equation to isolate k, which results in the units of k being \(\text{L mol}^{-1} \text{s}^{-1}\) for a second-order reaction.
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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 depends on the concentration of reactants. For example, a second-order reaction means that the rate is proportional to the square of the concentration of one reactant or the product of the concentrations of two reactants.
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Average Bond Order
Rate Constant (k)
The rate constant (k) is a proportionality factor in the rate law that relates the rate of a reaction to the concentrations of the reactants. Its units vary depending on the order of the reaction. For a second-order reaction, the units of k are typically expressed as M^-1 s^-1, indicating that the rate depends on the concentration squared.
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Units of Measurement in Chemistry
Units of measurement in chemistry are essential for quantifying concentrations, rates, and other properties. In the context of reaction kinetics, understanding how to derive the units of k based on the reaction order is crucial. For second-order reactions, the units of k reflect the need to balance the rate (M/s) with the concentration terms, leading to the specific units of M^-1 s^-1.
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Related Practice
Textbook Question
This graph shows a plot of the rate of a reaction versus the concentration of the reactant.
b. Make a rough sketch of a plot of [A] versus time
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?
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
Textbook Question
This graph shows a plot of the rate of a reaction versus the concentration of the reactant.
c. Write a rate law for the reaction including the value of k.
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. b. What would the rate of the reaction be at the concentration indicated in part a if the reaction were second order? Zero order? (Assume the same numerical value for the rate constant with the appropriate units.)
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