General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 17.9, Problem 17.15P
Write a balanced equation for the overall cell reaction when each of the following batteries is producing current:
- (a) Leclanché dry cell
- (b) Alkaline dry cell
- (c) Nickel–cadmium battery
- (d) Lithium battery
- (e) Lithium-ion battery
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionChapter 17 Solutions
General Chemistry: Atoms First
Ch. 17.1 - Describe a galvanic cell that uses the reaction...Ch. 17.2 - Write a balanced equation for the overall cell...Ch. 17.2 - Write the shorthand notation for a galvanic cell...Ch. 17.2 - Prob. 17.4CPCh. 17.3 - The standard cell potential at 25 C is 1.21 V for...Ch. 17.4 - The standard potential for the following galvanic...Ch. 17.5 - Which is the stronger oxidizing agent, Cl2(g) or...Ch. 17.5 - Predict from Table 17.1 whether each of the...Ch. 17.5 - Consider the following table of standard reduction...Ch. 17.6 - Consider a galvanic cell that uses the reaction...
Ch. 17.6 - Consider the following galvanic cell: (a) What is...Ch. 17.7 - What is the pH of the solution in the anode...Ch. 17.8 - Use the data in Table 17.1 to calculate the...Ch. 17.8 - Prob. 17.14PCh. 17.9 - Write a balanced equation for the overall cell...Ch. 17.10 - In what ways are fuel cells and batteries similar,...Ch. 17.10 - Prob. 17.17PCh. 17.11 - Prob. 17.18PCh. 17.12 - Metallic potassium was first prepared by Humphrey...Ch. 17.12 - Predict the half-cell reactions that occur when...Ch. 17.13 - Sketch an electrolytic cell suitable for...Ch. 17.14 - How many kilograms of aluminum can be produced in...Ch. 17.14 - A layer of silver is electroplated on a coffee...Ch. 17.14 - What is the overall cell reaction and cell...Ch. 17.14 - Prob. 17.25PCh. 17 - Prob. 17.26CPCh. 17 - Prob. 17.27CPCh. 17 - Prob. 17.28CPCh. 17 - Sketch a cell with inert electrodes suitable for...Ch. 17 - Prob. 17.30CPCh. 17 - It has recently been reported that porous pellets...Ch. 17 - Consider a Daniell cell with 1.0 M ion...Ch. 17 - Consider the following galvanic cell with 0.10 M...Ch. 17 - Prob. 17.34CPCh. 17 - Consider the following table of standard reduction...Ch. 17 - Prob. 17.36SPCh. 17 - What is the function of a salt bridge in a...Ch. 17 - Prob. 17.38SPCh. 17 - Describe galvanic cells that use the following...Ch. 17 - Write the standard shorthand notation for each...Ch. 17 - Write the standard shorthand notation for each...Ch. 17 - Prob. 17.42SPCh. 17 - Write the standard shorthand notation for a...Ch. 17 - An H2/H+ half-cell (anode) and an Ag+/Ag half-cell...Ch. 17 - A galvanic cell is constructed from a Zn/Zn2+...Ch. 17 - Prob. 17.46SPCh. 17 - Prob. 17.47SPCh. 17 - Prob. 17.48SPCh. 17 - Prob. 17.49SPCh. 17 - Prob. 17.50SPCh. 17 - Prob. 17.51SPCh. 17 - Prob. 17.52SPCh. 17 - Prob. 17.53SPCh. 17 - Prob. 17.54SPCh. 17 - Prob. 17.55SPCh. 17 - Prob. 17.56SPCh. 17 - Prob. 17.57SPCh. 17 - Prob. 17.58SPCh. 17 - Prob. 17.59SPCh. 17 - Prob. 17.60SPCh. 17 - Prob. 17.61SPCh. 17 - Prob. 17.62SPCh. 17 - Prob. 17.63SPCh. 17 - Prob. 17.64SPCh. 17 - Calculate E and G (in kilojoules) for the cell...Ch. 17 - Prob. 17.66SPCh. 17 - Prob. 17.67SPCh. 17 - Use the data in Appendix D to predict whether the...Ch. 17 - Use the data in Appendix D to predict whether the...Ch. 17 - Prob. 17.70SPCh. 17 - What reaction can occur, if any, when the...Ch. 17 - Consider a galvanic cell that uses the reaction...Ch. 17 - Prob. 17.73SPCh. 17 - Prob. 17.74SPCh. 17 - Prob. 17.75SPCh. 17 - Prob. 17.76SPCh. 17 - What is the Fe2+: Sn2+ concentration ratio in the...Ch. 17 - The Nernst equation applies to both cell reactions...Ch. 17 - Prob. 17.79SPCh. 17 - Prob. 17.80SPCh. 17 - Prob. 17.81SPCh. 17 - Prob. 17.82SPCh. 17 - Prob. 17.83SPCh. 17 - Prob. 17.84SPCh. 17 - Prob. 17.85SPCh. 17 - Prob. 17.86SPCh. 17 - Prob. 17.87SPCh. 17 - Calculate the equilibrium constant at 25 C for the...Ch. 17 - Prob. 17.89SPCh. 17 - For a lead storage battery: (a) Sketch one cell...Ch. 17 - Prob. 17.91SPCh. 17 - Prob. 17.92SPCh. 17 - Prob. 17.93SPCh. 17 - Prob. 17.94SPCh. 17 - Prob. 17.95SPCh. 17 - Prob. 17.96SPCh. 17 - Prob. 17.97SPCh. 17 - Prob. 17.98SPCh. 17 - (a)Sketch a cell with inert electrodes suitable...Ch. 17 - List the anode and cathode half-reactions that...Ch. 17 - Prob. 17.101SPCh. 17 - Prob. 17.102SPCh. 17 - Predict the anode, cathode, and overall cell...Ch. 17 - Prob. 17.104SPCh. 17 - Prob. 17.105SPCh. 17 - How many hours are required to produce 1.00 103...Ch. 17 - Prob. 17.107SPCh. 17 - Prob. 17.108SPCh. 17 - Prob. 17.109SPCh. 17 - Prob. 17.110CHPCh. 17 - Prob. 17.111CHPCh. 17 - Prob. 17.112CHPCh. 17 - Prob. 17.113CHPCh. 17 - Prob. 17.114CHPCh. 17 - Prob. 17.115CHPCh. 17 - Prob. 17.116CHPCh. 17 - Prob. 17.117CHPCh. 17 - Prob. 17.118CHPCh. 17 - The sodium-sulfur battery has molybdenum...Ch. 17 - When suspected drunk drivers are tested with a...Ch. 17 - Consider the addition of the following...Ch. 17 - The following galvanic cell has a potential of...Ch. 17 - A galvanic cell has a silver electrode in contact...Ch. 17 - Prob. 17.124CHPCh. 17 - Prob. 17.125CHPCh. 17 - Prob. 17.126CHPCh. 17 - For the following half-reaction, E = 1.103 V:...Ch. 17 - Prob. 17.128CHPCh. 17 - Prob. 17.129CHPCh. 17 - Prob. 17.130MPCh. 17 - Prob. 17.131MPCh. 17 - Prob. 17.134MPCh. 17 - Prob. 17.135MPCh. 17 - Prob. 17.136MPCh. 17 - Prob. 17.137MPCh. 17 - Experimental solid-oxide fuel cells that use...Ch. 17 - The half-reactions that occur in ordinary alkaline...Ch. 17 - Gold metal is extracted from its ore by treating...Ch. 17 - Consider the redox titration of 100.0 mL of a...
Knowledge Booster
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
- A mercury battery, used for hearing aids and electric watches, delivers a constant voltage (1.35 V) for long periods. The half-reactions are HgO(s)+H2O(l)+2eHg(l)+2OH(aq)Zn(s)+2OH(aq)Zn(OH)2(s)+2e Which half-reaction occurs at the anode and which occurs at the cathode? What is the overall cell reaction?arrow_forwardA galvanic cell is based on the following half-reactions at 25C: Ag++eAg H2O2+2H++2e2H2O Predict whether is larger or smaller than for the following cases. a. [Ag+]=1.0M,[H2O2]=2.0M,[H+]=2.0M b. [Ag+]=2.0M,[H2O2]=1.0M,[H+]=1.0107Marrow_forwardA potassium chloride solution is electrolyzed by passing a current through the solution using inert electrodes. A gas evolves at each electrode, and there is a large increase in pH of the solution. Write the half-reactions that occur at the anode and at the cathode.arrow_forward
- If alkaline batteries were not alkaline but rather acidic (as in the older dry cell batteries), what extra difficulties could you envision with corrosion, based on reactions that are part of the table of standard reduction potentials?arrow_forwardA voltaic cell is constructed from the following half-cells: a chromium electrode in chromium(III) sulfate solution and a lead electrode in lead(II) sulfate solution. The half-reactions are Cr(s)Cr3(aq)+3ePb2+(aq)+2ePb(s) Sketch the cell, labeling the anode and cathode (and the electrode reactions), and show the direction of electron flow and the movement of cations.arrow_forwardConsider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Introduction to Electrochemistry; Author: Tyler DeWitt;https://www.youtube.com/watch?v=teTkvUtW4SA;License: Standard YouTube License, CC-BY