Chemistry & Chemical Reactivity 10th Edition
ISBN: 9781337399074
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 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 19.9 Corrosion: Redox Reactions In The Environment 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 53PS: Use E values to predict which of the following metals, if coated on iron, will provide cathodic... Problem 54PS Problem 55PS Problem 56PS Problem 57GQ Problem 58GQ: Balance the following equations. (a) Zn(s) + VO2+(aq) Zn2+(aq) + V3+(aq)(acid solution) (b) Zn(s) +... Problem 59GQ: Magnesium metal is oxidized, and silver ions are reduced in a voltaic cell using Mg2+(aq, 1 M) | Mg... Problem 60GQ: You want to set up a series of voltaic cells with specific cell potentials. A Zn2+(aq, 1.0 M)| Zn(s)... Problem 61GQ Problem 62GQ Problem 63GQ: In the table of standard reduction potentials, locate the half-reactions for the reductions of the... Problem 64GQ Problem 65GQ: Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode. The... Problem 66GQ: The following half-cells are available: (i) Ag+(aq, 1.0M)|Ag(s) (ii) Zn2+(aq, 1.0 M) |Zn(s) (iii)... Problem 67GQ Problem 68GQ Problem 69GQ: A potential of 0.142 V is recorded (under standard conditions) for a voltaic cell constructed using... Problem 70GQ Problem 71GQ: The standard potential, E, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard... Problem 72GQ: An electrolysis cell for aluminum production operates at 5.0 V and a current of 1.0 105 A.... Problem 73GQ: Electrolysis of molten NaCl is done in cells operating at 7.0 V and 4.0 104 A. What mass of Na(s)... Problem 74GQ: A current of 0.0100 A is passed through a solution of rhodium sulfate, causing reduction of the... Problem 75GQ: A current of 0.44 A is passed through a solution of ruthenium nitrate causing reduction of the metal... Problem 76GQ Problem 77GQ Problem 78GQ Problem 79GQ: The products formed in the electrolysis of aqueous CuSO4 are Cu(s) and O2(g). Write equations for... Problem 80GQ: Predict the products formed in the electrolysis of an aqueous solution of CdSO4. Problem 81GQ Problem 82GQ: The metallurgy of aluminum involves electrolysis of Al2O3 dissolved in molten cryolite (Na3AlF6) at... Problem 83GQ Problem 84GQ Problem 85GQ Problem 86GQ Problem 87GQ: Two Ag+(aq) | Ag(s) half-cells are constructed. The first has [Ag+] = 1.0 M, the second has [Ag+] =... Problem 88GQ: Calculate equilibrium constants for the following reactions at 208 K. Indicate whether the... Problem 89GQ Problem 90GQ: Use the table of standard reduction potentials (Appendix M) to calculate rG for the following... Problem 91GQ Problem 92GQ Problem 93GQ Problem 94GQ: A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous... Problem 95GQ: An expensive but lighter alternative to the lead storage battery is the silver-zinc battery. Ag2O(s)... Problem 96GQ: The specifications for a lead storage battery include delivery of a steady 1.5 A of current for 15... Problem 97GQ: Manganese may play an important role in chemical cycles in the oceans. Two reactions involving... Problem 98GQ Problem 99GQ: Iron(II) ion undergoes a disproportionation reaction to give Fe(s) and the iron(III) ion. That is,... Problem 100GQ: Copper(I) ion disproportionates to copper metal and copper(ll) ion. (See Study Question 99.) 2... Problem 101GQ Problem 102GQ Problem 103GQ: Can either sodium or potassium metal be used as a sacrificial anode to protect the iron hull of a... Problem 104GQ: Galvanized steel pipes are used in the plumbing of many older homes. When copper plumbing is added... Problem 105IL: Consider an electrochemical cell based on the half-reactions Ni2+(aq) + 2 e Ni(s) and Cd2+(aq) + 2e... Problem 106IL Problem 107IL: A silver coulometer (Study Question 106) was used in the past to measure the current flowing in an... Problem 108IL: Four metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M... Problem 109IL Problem 110IL: The amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The... Problem 111SCQ Problem 112SCQ: The free energy change for a reaction, rG, is the maximum energy that can be extracted from the... Problem 113SCQ Problem 114SCQ: (a) Is it easier to reduce water in acid or base? To evaluate this, consider the half-reaction... Problem 115SCQ Problem 33PS: One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of...
Related questions
Voltaic cell and Electrolysis
Transcribed Image Text: VOLTAIC CELL AND ELECTROLYSIS
A voltaic cell was constructed based on the two reactions shown below:
Reduction half reaction: Cl2(aq) + 2 e² → Cl-
Oxidation half reaction: Al(s) A1³+ (aq) + 3 e¯
Ereduction
Eº
1.36 V
oxidation = 1.66 V
1. Balance the oxidation half reaction (OHR)
2. Balance the reduction half reaction (RHR)
3. Write the overall reaction.
4. Determine the standard cell potential of the constructed voltaic cell.
5. What is the cell potential if [CI] = 0.75 M and [A1³+] = 0.50 M? Assume that the experiment
was done at 25.0°C.
Definition Definition Process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 6 steps with 4 images
![VOLTAIC CELL AND ELECTROLYSIS
A voltaic cell was constructed based on the two reactions shown below:
Reduction half reaction: Cl2(aq) + 2 e² → Cl-
Oxidation half reaction: Al(s) A1³+ (aq) + 3 e¯
Ereduction
Eº
1.36 V
oxidation = 1.66 V
1. Balance the oxidation half reaction (OHR)
2. Balance the reduction half reaction (RHR)
3. Write the overall reaction.
4. Determine the standard cell potential of the constructed voltaic cell.
5. What is the cell potential if [CI] = 0.75 M and [A1³+] = 0.50 M? Assume that the experiment
was done at 25.0°C.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F409b9142-20d9-4f17-9785-47022f000408%2F0ec778eb-a95a-4d29-b31c-6dd2b1a3214b%2F6pq5y7e_processed.jpeg&w=3840&q=75)
