The reaction that occurs in a lead-acid battery is as follows:
What gets oxidized is this battery? What gets reduced? What is the oxidizing agent? What is the reducing agent?
Want to see the full answer?
Check out a sample textbook solutionChapter 14 Solutions
EBK INTRODUCTION TO CHEMISTRY
- An electrolytic cell is set up with Cd(s) in Cd(NO3)2(aq) and Zn(s) in Zn(NO3)2(aq). Initially both electrodesweigh 5.00 g. After running the cell for several hours theelectrode in the left compartment weighs 4.75 g. (a) Which electrode is in the left compartment? (b) Does the mass of the electrode in the right compartmentincrease, decrease, or stay the same? If the masschanges, what is the new mass? (c) Does the volume of the electrode in the right compartment increase, decrease, or stay the same? If the volumechanges, what is the new volume? (The density of Cd is8.65 g/cm3.)arrow_forwardConsider the following galvanic cell: Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is dead.arrow_forwardConsider these half-reactions: (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Sn(s) reduce Ag+(aq) to Ag(s)? (f) Will Hg() reduce Sn2+(aq) to Sn(s)? (g) Name the ions that can be reduced by Sn(s). (h) Which metals can be oxidized by Ag+(aq)?arrow_forward
- Draw a diagram of each cell. Label the anode, the cathode, the species in each half-cell solution, the direction of electron movement in an external circuit, and thedirection of movement of ions within the cell. (a) Cu(s) | Cu2+(aq) || Fe2+(aq) |Fe(s) (b) Pt(s) | H2O2(aq), H+(aq) || Fe2+(aq), Fe3+(aq) | Pt(s)arrow_forwardFor the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+ (aq), why can’t you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing CuCl2(aq) and ZnCl2(aq)?arrow_forwardThe voltaic cell is represented as Zn(s)Zn2+(1.0M)Cu2+(1.0M)Cu(s) Which of the following statements is not true of this cell? a The mass of the zinc electrode, Zn(s), decreases as the cell runs. b The copper electrode is the anode. c Electrons flow through the external circuit from the zinc electrode to the copper electrode. d Reduction occurs at the copper electrode as the cell runs. e The concentration of Cu2+ decreases as the cell runs.arrow_forward
- Use Table 17.1 to arrange the following oxidizing agents in order of increasing strength: Mn2+ S Co3+ Cl2 K+arrow_forwardDescribe what you expect to happen when the following solutions are electrolyzed: a aqueous Na2SO4; b aqueous KBr. That is, what are the electrode reactions? What is the overall reaction?arrow_forwardWhen molten lithium chloride, LiCl, is electrolyzed, lithium metal is liberated at the cathode. How many grams of lithium are liberated when 2.00 103 C of charge passes through the cell?arrow_forward
- Four metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (b) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (c) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.arrow_forwardWrite balanced equations for the following half-reactions. Specify whether each is an oxidation or reduction. (a) H2O2(aq) O2(g)(in acid) (b) H2C2O4(aq) CO2(g)(in acid) (c) NO3(aq) NO(g)(in acid) (d) MnO4(aq) MnO2(s)(in base)arrow_forwardWhat is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning