Homework Help is Here – Start Your Trial Now!
Science
Chemistry
cell A B C n 1 1 1 calculated quantities (Check the box next to any that are wrong.) 0 AGⓇ -81. kJ/mol -80. kJ/mol 145. kJ/mol K 6.45 × 10 14 1.04 X 10 -15 25 2.53 × 10 0 E -0.84 V -0.83 V -1.50 V O O O

cell A B C n 1 1 1 calculated quantities (Check the box next to any that are wrong.) 0 AGⓇ -81. kJ/mol -80. kJ/mol 145. kJ/mol K 6.45 × 10 14 1.04 X 10 -15 25 2.53 × 10 0 E -0.84 V -0.83 V -1.50 V O O O

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
A student made measurements on some electrochemical cells and calculated three quantities: - The standard reaction free energy \( \Delta G^0 \). - The equilibrium constant \( K \) at 25.0 \( ^\circ C \). - The cell potential under standard conditions \( E^0 \). His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. **Note:** If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. **Also note:** for each cell, the number \( n \) of electrons transferred per redox reaction is 1.
Transcribed Image Text:A student made measurements on some electrochemical cells and calculated three quantities: - The standard reaction free energy \( \Delta G^0 \). - The equilibrium constant \( K \) at 25.0 \( ^\circ C \). - The cell potential under standard conditions \( E^0 \). His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. **Note:** If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. **Also note:** for each cell, the number \( n \) of electrons transferred per redox reaction is 1.
**Transcription and Explanation for Educational Website:** --- **Note:** For each cell, the number of electrons transferred per redox reaction is 1. --- ### Table: Calculated Quantities **Instruction:** Check the box next to any quantities that are incorrect. | **Cell** | **n** | \(\Delta G^{0}\) (kJ/mol) | \(K\) | \(E^{0}\) (V) | |----------|-------|-----------------------------|-----------------------------------------|---------------| | A | 1 | \(-81\) | \(6.45 \times 10^{-15}\) | \(-0.84\) | | B | 1 | \(-80\) | \(1.04 \times 10^{14}\) | \(-0.83\) | | C | 1 | \(145\) | \(2.53 \times 10^{25}\) | \(-1.50\) | *Note: A checkbox is checked next to \(\Delta G^{0} = -81 \, \text{kJ/mol}\) for Cell A, indicating a potential error in the calculation of this value.* **Explanation:** - **\(\Delta G^{0}\)** represents the standard Gibbs free energy change for the reaction in each cell, measured in kilojoules per mole (kJ/mol). - **\(K\)** is the equilibrium constant, indicating the favorability of the reaction under standard conditions. - **\(E^{0}\)** is the standard cell potential, measured in volts (V), a measure of the electromotive force of the cell. This table is used to compare the thermodynamic properties of different electrochemical cells and identify any discrepancies in the calculated quantities.
Transcribed Image Text:**Transcription and Explanation for Educational Website:** --- **Note:** For each cell, the number of electrons transferred per redox reaction is 1. --- ### Table: Calculated Quantities **Instruction:** Check the box next to any quantities that are incorrect. | **Cell** | **n** | \(\Delta G^{0}\) (kJ/mol) | \(K\) | \(E^{0}\) (V) | |----------|-------|-----------------------------|-----------------------------------------|---------------| | A | 1 | \(-81\) | \(6.45 \times 10^{-15}\) | \(-0.84\) | | B | 1 | \(-80\) | \(1.04 \times 10^{14}\) | \(-0.83\) | | C | 1 | \(145\) | \(2.53 \times 10^{25}\) | \(-1.50\) | *Note: A checkbox is checked next to \(\Delta G^{0} = -81 \, \text{kJ/mol}\) for Cell A, indicating a potential error in the calculation of this value.* **Explanation:** - **\(\Delta G^{0}\)** represents the standard Gibbs free energy change for the reaction in each cell, measured in kilojoules per mole (kJ/mol). - **\(K\)** is the equilibrium constant, indicating the favorability of the reaction under standard conditions. - **\(E^{0}\)** is the standard cell potential, measured in volts (V), a measure of the electromotive force of the cell. This table is used to compare the thermodynamic properties of different electrochemical cells and identify any discrepancies in the calculated quantities.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Photochemistry
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