Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Using the information from the table below, what should be the unit for k? Total reaction order 0 1 2 di 3 multiple sma products a Units of k mol/(L-s) 1/s or s-1 L/(mol-s) L²/(mol²-s) form of rate of ents decrease (called the elementary steps), an complex, which

Using the information from the table below, what should be the unit for k? Total reaction order 0 1 2 di 3 multiple sma products a Units of k mol/(L-s) 1/s or s-1 L/(mol-s) L²/(mol²-s) form of rate of ents decrease (called the elementary steps), an complex, which

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
### Understanding Units for the Rate Constant (k) Based on Reaction Order When studying reaction kinetics, it is essential to determine the appropriate units for the rate constant (k) based on the total reaction order. The table below provides a summary of the units for k for different reaction orders: #### Table: Units of the Rate Constant (k) for Different Reaction Orders | Total Reaction Order | Units of k | |----------------------|-------------------------| | 0 | mol/(L·s) | | 1 | 1/s or s⁻¹ | | 2 | L/(mol·s) | | 3 | L²/(mol²·s) | **Interpreting the Table:** - **Zero-order reaction (0):** The rate of reaction is independent of the concentration of the reactants. The units for k are mol/(L·s), indicating the rate is in moles per liter per second. - **First-order reaction (1):** The rate of reaction is directly proportional to the concentration of one reactant. The units for k are 1/s or s⁻¹, meaning the rate is per second. - **Second-order reaction (2):** The rate is proportional to the product of the concentrations of two reactants or the square of the concentration of one reactant. The units for k are L/(mol·s), indicating liter per mole per second. - **Third-order reaction (3):** The rate is proportional to the product of the concentrations of three reactants or the cube of the concentration of one reactant. The units for k are L²/(mol²·s), indicating liters squared per mole squared per second. Using this information, you can determine the unit for k based on the reaction order of the chemical reaction you are studying. In chemical kinetics, understanding the units of the rate constant is crucial for analyzing and interpreting the rate laws and mechanisms of reactions. Depending on how the concentrations of reactants influence the reaction rate, the units of k vary, reflecting the different dependencies on concentration. ### Application Example: Suppose you are given a reaction and need to determine the appropriate unit for the rate constant k. Identify the reaction order and refer to the table to find the corresponding unit for k. For instance, if you have a third-order reaction, the unit for k would be L²/(mol²·s).
Transcribed Image Text:### Understanding Units for the Rate Constant (k) Based on Reaction Order When studying reaction kinetics, it is essential to determine the appropriate units for the rate constant (k) based on the total reaction order. The table below provides a summary of the units for k for different reaction orders: #### Table: Units of the Rate Constant (k) for Different Reaction Orders | Total Reaction Order | Units of k | |----------------------|-------------------------| | 0 | mol/(L·s) | | 1 | 1/s or s⁻¹ | | 2 | L/(mol·s) | | 3 | L²/(mol²·s) | **Interpreting the Table:** - **Zero-order reaction (0):** The rate of reaction is independent of the concentration of the reactants. The units for k are mol/(L·s), indicating the rate is in moles per liter per second. - **First-order reaction (1):** The rate of reaction is directly proportional to the concentration of one reactant. The units for k are 1/s or s⁻¹, meaning the rate is per second. - **Second-order reaction (2):** The rate is proportional to the product of the concentrations of two reactants or the square of the concentration of one reactant. The units for k are L/(mol·s), indicating liter per mole per second. - **Third-order reaction (3):** The rate is proportional to the product of the concentrations of three reactants or the cube of the concentration of one reactant. The units for k are L²/(mol²·s), indicating liters squared per mole squared per second. Using this information, you can determine the unit for k based on the reaction order of the chemical reaction you are studying. In chemical kinetics, understanding the units of the rate constant is crucial for analyzing and interpreting the rate laws and mechanisms of reactions. Depending on how the concentrations of reactants influence the reaction rate, the units of k vary, reflecting the different dependencies on concentration. ### Application Example: Suppose you are given a reaction and need to determine the appropriate unit for the rate constant k. Identify the reaction order and refer to the table to find the corresponding unit for k. For instance, if you have a third-order reaction, the unit for k would be L²/(mol²·s).
Expert Solution
steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Rate Laws
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS