Chemistry & Chemical Reactivity 9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
1 Basic Concepts Of Chemistry 2 Atoms Molecules And Ions 3 Chemical Reactions 4 Stoichiometry: Quantitative Information About Chemical Reactions 5 Principles Of Chemical Reactivity: Energy And Chemical Reactions 6 The Structure Of Atoms 7 The Structure Of Atoms And Periodic Trends 8 Bonding And Molecular Structure 9 Bonding And Molecular Structure: Orbital Hybridization And Molecular Orbitals 10 Gases And Their Properties 11 Intermolecular Forces And Liquids 12 The Solid State 13 Solutions And Their Behavior 14 Chemical Kinetics: The Rates Of Chemical Reactions 15 Principles Of Chemical Reactivity: Equilibria 16 Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases 17 Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria 18 Principles Of Chemical Reactivity: Entropy And Free Energy 19 Principles Of Chemical Reactivity: Electron Transfer Reactions 20 Environmental Chemistry-earth's Environment, Energy, And Sustainability 21 The Chemistry Of The Main Group Elements 22 The Chemistry Of The Transistion Elements 23 Carbon: Not Just Another Element 24 Biochemistry 25 Nuclear Chemistry L Let's Review Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
19.1 Oxidation-reduction Reactions 19.2 Simple Voltaic Cells 19.3 Commerical Voltaic Cells 19.4 Standard Electrochemical Potentials 19.5 Electrochemical Cells Under Nonstandard Conditions 19.6 Electrochemistry And Thermodynamics 19.7 Electrolysis: Chemical Change Using Electrical Energy 19.8 Counting Electrons Chapter Questions Section: Chapter Questions
Problem 1PS: Write balanced equations for the following half-reactions. Specify whether each is an oxidation or... Problem 2PS: Write balanced equations for the following half-reactions. Specify whether each is an oxidation or... Problem 3PS: Balance the following redox equations. All occur in acid solution. (a) Ag(s) + NO3(aq) NO2(g) +... Problem 4PS: Balance the following redox equations. All occur in acid solution. (a) Sn(s) + H+(aq) Sn2+(aq) +... Problem 5PS: Balance the following redox equations. All occur in basic solution. (a) Al(s) + H2O() Al(OH)4(aq) +... Problem 6PS Problem 7PS: A voltaic cell is constructed using the reaction of chromium metal and iron(II) ions. 2 Cr(s) + 3... Problem 8PS: A voltaic cell is constructed using the reaction Mg(s) + 2H+(aq) Mg2+(aq) + H2(g) (a) Write... Problem 9PS: The half-cells Fe2+(aq) | Fe(s) and O2(g) | H2O (in and solution) are linked to create a voltaic... Problem 10PS: The half cells Sn2+(aq) |Sn(s) and Cl2(g) |Cl(aq) are linked to create a voltaic cell. (a) Write... Problem 11PS: For each of the following electrochemical cells, write equations for the oxidation and reduction... Problem 12PS: For each of the following electrochemical cells, write equations for lire oxidation and reduction... Problem 13PS: Use cell notation to depict an electrochemical cell based upon the following reaction that is... Problem 14PS: Use cell notation to depict an electrochemical cell based upon the following reaction that is... Problem 15PS: What are the similarities and differences between dry cells, alkaline batteries, and Ni-cad... Problem 16PS: What reactions occur when a lead storage battery is recharged? Problem 17PS: Calculate the value of E for each of the following reactions. Decide whether each is product-favored... Problem 18PS: Calculate the value of E for each of the following reactions. Decide whether each is product-favored... Problem 19PS: Balance each of the following unbalanced equations; then calculate the standard potential, E, and... Problem 20PS: Balance each of the following unbalanced equations; then calculate the standard potential, E, and... Problem 21PS: Consider the following half-reactions: (a) Based on E values, which metal is the mosteasily... Problem 22PS Problem 23PS: Which of the following elements is the best reducing agent under standard conditions? (a) Cu (b) Zn... Problem 24PS Problem 25PS: Which of the following ions is most easily reduced? (a) Cu2+(aq) (b) Zn2+(aq) (c) Fe2+(aq) (d)... Problem 26PS: From the following list, identify the ions that are more easily reduced than H+(aq). (a) Cu2+(aq)... Problem 27PS: (a) Which halogen is most easily reduced in acidic solution: F2, Cl2, Br., or I2? (b) Identify the... Problem 28PS Problem 29PS: Calculate the potential delivered by a voltaic cell using the following reaction if all dissolved... Problem 30PS: Calculate the potential developed by a voltaic cell using the following reaction if all dissolved... Problem 31PS: One half-cell in a voltaic cell is constructed from a silver wire electrode in a 0.25 M solution of... Problem 32PS: One half-cell in a voltaic cell is constructed from a copper wire electrode in a 4.8 103 M solution... Problem 33PS: One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of... Problem 34PS: One half-cell in a voltaic cell is constructed from an iron electrode in an Fe(NO3)2 solution of... Problem 35PS: Calculate rG and the equilibrium constant for the following reactions. (a) 2 Fe3+(aq) + 2 I(aq) 2... Problem 36PS Problem 37PS: Use standard reduction potentials (Appendix M) for the half-reactions AgBr(s) + e Ag(s) + Br(aq)... Problem 38PS: Use the standard reduction potentials (Appendix M) for the half-reactions Hg2Cl2(s) + 2 e 2 Hg() +... Problem 39PS: Use the standard reduction potentials (Appendix M) for the half-reactions [AuCl4](aq) + 3 e Au(s) +... Problem 40PS: Use the standard reduction potentials (Appendix M) for the half reactions [Zn(OH)4]2(aq) + 2 e Zn... Problem 41PS Problem 42PS Problem 43PS: Which product, O2 or F2, is more likely to form at the anode in the electrolysis of an aqueous... Problem 44PS: Which product, Ca or H2, is more likely to form at the cathode in the electrolysis of CaCl2? Explain... Problem 45PS: An aqueous solution of KBr is placed in a beaker with two inert platinum electrodes. When the cell... Problem 46PS: An aqueous solution of Na2S is placed in a beaker with two inert platinum electrodes. When the cell... Problem 47PS: In the electrolysis of a solution containing Ni2+(aq), metallic Ni(s) deposits on the cathode. Using... Problem 48PS: In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using... Problem 49PS: Electrolysis of a solution of CuSO4(aq) to give copper metal is carried out using a current of 0.66... Problem 50PS: Electrolysis of a solution of Zn(NO3)2(aq) to give zinc metal is carried out using a current of 2.12... Problem 51PS: A voltaic cell can be built using the reaction between Al metal and O2 from the air. If the Al anode... Problem 52PS: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.25 A of current for 1.00... Problem 53GQ Problem 54GQ: Balance the following equations. (a) Zn(s) + VO2+(aq) Zn2+(aq) + V3+(aq)(acid solution) (b) Zn(s) +... Problem 55GQ: Magnesium metal is oxidized, and silver ions are reduced in a voltaic cell using Mg2+(aq, 1 M) | Mg... Problem 56GQ: You want to set up a series of voltaic cells with specific cell potentials. A Zn2+(aq, 1.0 M)| Zn(s)... Problem 57GQ Problem 58GQ Problem 59GQ: In the table of standard reduction potentials, locate the half-reactions for the reductions of the... Problem 60GQ Problem 61GQ: Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode. The... Problem 62GQ: The following half-cells are available: (i) Ag+(aq, 1.0M)|Ag(s) (ii) Zn2+(aq, 1.0 M) |Zn(s) (iii)... Problem 63GQ Problem 64GQ Problem 65GQ: A potential of 0.142 V is recorded (under standard conditions) for a voltaic cell constructed using... Problem 66GQ Problem 67GQ: The standard potential, E, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard... Problem 68GQ: An electrolysis cell for aluminum production operates at 5.0 V and a current of 1.0 105 A.... Problem 69GQ: Electrolysis of molten NaCl is done in cells operating at 7.0 V and 4.0 104 A. What mass of Na(s)... Problem 70GQ: A current of 0.0100 A is passed through a solution of rhodium sulfate, causing reduction of the... Problem 71GQ: A current of 0.44 A is passed through a solution of ruthenium nitrate causing reduction of the metal... Problem 72GQ Problem 73GQ Problem 74GQ Problem 75GQ: The products formed in the electrolysis of aqueous CuSO4 are Cu(s) and O2(g). Write equations for... Problem 76GQ: Predict the products formed in the electrolysis of an aqueous solution of CdSO4. Problem 77GQ Problem 78GQ: The metallurgy of aluminum involves electrolysis of Al2O3 dissolved in molten cryolite (Na3AlF6) at... Problem 79GQ Problem 80GQ Problem 81GQ Problem 82GQ Problem 83GQ: Two Ag+(aq) | Ag(s) half-cells are constructed. The first has [Ag+] = 1.0 M, the second has [Ag+] =... Problem 84GQ: Calculate equilibrium constants for the following reactions at 208 K. Indicate whether the... Problem 85GQ Problem 86GQ: Use the table of standard reduction potentials (Appendix M) to calculate rG for the following... Problem 87GQ Problem 88GQ Problem 89GQ Problem 90GQ: A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous... Problem 91GQ: An expensive but lighter alternative to the lead storage battery is the silver-zinc battery. Ag2O(s)... Problem 92GQ: The specifications for a lead storage battery include delivery of a steady 1.5 A of current for 15... Problem 93GQ: Manganese may play an important role in chemical cycles in the oceans. Two reactions involving... Problem 94GQ Problem 95GQ: Iron(II) ion undergoes a disproportionation reaction to give Fe(s) and the iron(III) ion. That is,... Problem 96GQ: Copper(I) ion disproportionates to copper metal and copper(ll) ion. (See Study Question 99.) 2... Problem 97GQ Problem 98GQ Problem 99IL: Consider an electrochemical cell based on the half-reactions Ni2+(aq) + 2 e Ni(s) and Cd2+(aq) + 2e... Problem 100IL Problem 101IL: A silver coulometer (Study Question 106) was used in the past to measure the current flowing in an... Problem 102IL: Four metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M... Problem 103IL Problem 104IL: The amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The... Problem 105SCQ Problem 106SCQ: The free energy change for a reaction, rG, is the maximum energy that can be extracted from the... Problem 107SCQ Problem 108SCQ: (a) Is it easier to reduce water in acid or base? To evaluate this, consider the half-reaction... Problem 109SCQ Problem 8PS: A voltaic cell is constructed using the reaction Mg(s) + 2H+(aq) Mg2+(aq) + H2(g) (a) Write...
Given the cell notation for a redox reaction, give the balanced overall redox reaction. How do you go about that problem? Can you explain in detail?
Transcribed Image Text: Example 17.3
Using Cell Notation
Consider a galvanic cell consisting of
2Cr(s) + 3Cu²+(aq) → 2Cr³+ (aq) + 3Cu(s)
Write the oxidation and reduction half-reactions and write the reaction using cell notation. Which reaction
occurs at the anode? The cathode?
oxidation:
2 Cr(s)
reduction: 3 Cu2+ (aq) + 6e-
2 Cr3+(aq) + 6e-
3 Cu(s)
The oxidation reaction (Cr (s) → Cr3+) occurs at the anode
The reduction reaction (Cu2+ Cu(s)) occurs at the cathode
Cell Notation:
Cr (s) | Cr3+ (aq) || Cu2+ (aq) | Cu (s)
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
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