Chemistry & Chemical Reactivity, Hybrid Edition (with OWLv2 24-Months Printed Access Card)
Chemistry & Chemical Reactivity, Hybrid Edition (with OWLv2 24-Months Printed Access Card)
9th Edition
ISBN: 9781285462530
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 19, Problem 88GQ

(a)

Interpretation Introduction

Interpretation:

A balanced equation for the following reaction has to be determined.

(a) HCO2 CH2O                           (acid solution)

Concept introduction:

Oxidation reaction:

The loss of electrons or the gain of oxigen atoms.And also increase their oxidation number.

Ag  Ag++ e-

In the above reaction , Ag atom lose one electron and change their oxidation state 0 to 1.

Reduction reaction:

Gaining electrons or adding hydrogen atoms. And also decrease their oxidation number.

Fe2++2e-  Fe

In the above reaction Fe2+ ion gaining 2 electrons and reduce their oxidation number +2 to 0.

Steps for balancing reactions in ACIDIC solution:

  1. 1. Balance all atoms except H and O in half reaction.
  2. 2. Balance O atoms by adding water to the side missing O atoms.
  3. 3. Balance the H atoms by adding H+ to the side missing H atoms.
  4. 4. Balance the charge by adding electrons to side with more total positive charge.
  5. 5. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.

Steps for balancing reactions in BASIC solution:

  1. 1. Balance all atoms except H and O in half reaction.
  2. 2. Balance O atoms by adding water to the side missing O atoms.
  3. 3. Balance the H atoms by adding H+ to the side missing H atoms.
  4. 4. Balance the charge by adding electrons to side with more total positive charge.
  5. 5. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.
  6. 6. Add the same number of OH- groups as there are H+ present to both sides of the equation.

(b)

Interpretation Introduction

Interpretation:

A balanced equation for the following reaction has to be determined.

(b) C6H5CO2 C6H5CH3               (acid solution)

Concept introduction:

Oxidation reaction:

The loss of electrons or the gain of oxigen atoms.And also increase their oxidation number.

Ag  Ag++ e-

In the above reaction , Ag atom lose one electron and change their oxidation state 0 to 1.

Reduction reaction:

Gaining electrons or adding hydrogen atoms. And also decrease their oxidation number.

Fe2++2e-  Fe

In the above reaction Fe2+ ion gaining 2 electrons and reduce their oxidation number +2 to 0.

Steps for balancing reactions in ACIDIC solution:

  1. 6. Balance all atoms except H and O in half reaction.
  2. 7. Balance O atoms by adding water to the side missing O atoms.
  3. 8. Balance the H atoms by adding H+ to the side missing H atoms.
  4. 9. Balance the charge by adding electrons to side with more total positive charge.
  5. 10. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.

Steps for balancing reactions in BASIC solution:

  1. 7. Balance all atoms except H and O in half reaction.
  2. 8. Balance O atoms by adding water to the side missing O atoms.
  3. 9. Balance the H atoms by adding H+ to the side missing H atoms.
  4. 10. Balance the charge by adding electrons to side with more total positive charge.
  5. 11. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.
  6. 12. Add the same number of OH- groups as there are H+ present to both sides of the equation.

(c)

Interpretation Introduction

Interpretation:

A balanced equation for the following reaction has to be determined.

(c) CH3CH2CHO CH3CH2CH2OH (acid solution)

Concept introduction:

Oxidation reaction:

The loss of electrons or the gain of oxigen atoms.And also increase their oxidation number.

Ag  Ag++ e-

In the above reaction , Ag atom lose one electron and change their oxidation state 0 to 1.

Reduction reaction:

Gaining electrons or adding hydrogen atoms. And also decrease their oxidation number.

Fe2++2e-  Fe

In the above reaction Fe2+ ion gaining 2 electrons and reduce their oxidation number +2 to 0.

Steps for balancing reactions in ACIDIC solution:

  1. 11. Balance all atoms except H and O in half reaction.
  2. 12. Balance O atoms by adding water to the side missing O atoms.
  3. 13. Balance the H atoms by adding H+ to the side missing H atoms.
  4. 14. Balance the charge by adding electrons to side with more total positive charge.
  5. 15. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.

Steps for balancing reactions in BASIC solution:

  1. 13. Balance all atoms except H and O in half reaction.
  2. 14. Balance O atoms by adding water to the side missing O atoms.
  3. 15. Balance the H atoms by adding H+ to the side missing H atoms.
  4. 16. Balance the charge by adding electrons to side with more total positive charge.
  5. 17. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.
  6. 18. Add the same number of OH- groups as there are H+ present to both sides of the equation.

(d)

Interpretation Introduction

Interpretation:

A balanced equation for the following reaction has to be determined.

(d)CH3OH  CH4                              (acid solution)

Concept introduction:

Oxidation reaction:

The loss of electrons or the gain of oxigen atoms.And also increase their oxidation number.

Ag  Ag++ e-

In the above reaction , Ag atom lose one electron and change their oxidation state 0 to 1.

Reduction reaction:

Gaining electrons or adding hydrogen atoms. And also decrease their oxidation number.

Fe2++2e-  Fe

In the above reaction Fe2+ ion gaining 2 electrons and reduce their oxidation number +2 to 0.

Steps for balancing reactions in ACIDIC solution:

  1. 16. Balance all atoms except H and O in half reaction.
  2. 17. Balance O atoms by adding water to the side missing O atoms.
  3. 18. Balance the H atoms by adding H+ to the side missing H atoms.
  4. 19. Balance the charge by adding electrons to side with more total positive charge.
  5. 20. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.

Steps for balancing reactions in BASIC solution:

  1. 19. Balance all atoms except H and O in half reaction.
  2. 20. Balance O atoms by adding water to the side missing O atoms.
  3. 21. Balance the H atoms by adding H+ to the side missing H atoms.
  4. 22. Balance the charge by adding electrons to side with more total positive charge.
  5. 23. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.
  6. 24. Add the same number of OH- groups as there are H+ present to both sides of the equation.

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Chapter 19 Solutions

Chemistry & Chemical Reactivity, Hybrid Edition (with OWLv2 24-Months Printed Access Card)

Ch. 19.3 - Prob. 1RCCh. 19.3 - Prob. 2RCCh. 19.4 - (a) Rank the following metals in their ability to...Ch. 19.4 - Prob. 1RCCh. 19.4 - Prob. 2RCCh. 19.4 - Prob. 3RCCh. 19.4 - Prob. 1QCh. 19.4 - Prob. 2QCh. 19.4 - Prob. 3QCh. 19.5 - A voltaic cell is set up with an aluminum...Ch. 19.5 - Check Your Understanding The half-cells Fe2+(aq,...Ch. 19.5 - Prob. 1RCCh. 19.6 - Prob. 1CYUCh. 19.6 - Calculate the equilibrium constant at 25 C for the...Ch. 19.6 - Prob. 1RCCh. 19.7 - Predict the chemical reactions that will occur at...Ch. 19.7 - Prob. 1RCCh. 19.8 - Prob. 1CYUCh. 19.8 - 1. If you wish to convert 0.0100 mol of Au3+ (aq)...Ch. 19.8 - Prob. 1QCh. 19.8 - Use standard reduction potentials to determine...Ch. 19.8 - Prob. 3QCh. 19.8 - The overall reaction for the production of Cu(OH)2...Ch. 19.8 - Assume the following electrochemical cell...Ch. 19 - Write balanced equations for the following...Ch. 19 - Write balanced equations for the following...Ch. 19 - Balance the following redox equations. All occur...Ch. 19 - Balance the following redox equations. All occur...Ch. 19 - Balance the following redox equations. All occur...Ch. 19 - Prob. 6PSCh. 19 - A voltaic cell is constructed using the reaction...Ch. 19 - A voltaic cell is constructed using the reaction...Ch. 19 - The half-cells Fe2+(aq) | Fe(s) and O2(g) | H2O...Ch. 19 - The half cells Sn2+(aq) |Sn(s) and Cl2(g) |Cl(aq)...Ch. 19 - For each of the following electrochemical cells,...Ch. 19 - For each of the following electrochemical cells,...Ch. 19 - Use cell notation to depict an electrochemical...Ch. 19 - Use cell notation to depict an electrochemical...Ch. 19 - What are the similarities and differences between...Ch. 19 - What reactions occur when a lead storage battery...Ch. 19 - Calculate the value of E for each of the following...Ch. 19 - Calculate the value of E for each of the following...Ch. 19 - Balance each of the following unbalanced...Ch. 19 - Balance each of the following unbalanced...Ch. 19 - Consider the following half-reactions: (a) Based...Ch. 19 - Prob. 22PSCh. 19 - Which of the following elements is the best...Ch. 19 - Prob. 24PSCh. 19 - Which of the following ions is most easily...Ch. 19 - From the following list, identify the ions that...Ch. 19 - (a) Which halogen is most easily reduced in acidic...Ch. 19 - Prob. 28PSCh. 19 - Calculate the potential delivered by a voltaic...Ch. 19 - Calculate the potential developed by a voltaic...Ch. 19 - One half-cell in a voltaic cell is constructed...Ch. 19 - One half-cell in a voltaic cell is constructed...Ch. 19 - One half-cell in a voltaic cell is constructed...Ch. 19 - One half-cell in a voltaic cell is constructed...Ch. 19 - Calculate rG and the equilibrium constant for the...Ch. 19 - Prob. 36PSCh. 19 - Use standard reduction potentials (Appendix M) for...Ch. 19 - Use the standard reduction potentials (Appendix M)...Ch. 19 - Use the standard reduction potentials (Appendix M)...Ch. 19 - Use the standard reduction potentials (Appendix M)...Ch. 19 - Prob. 41PSCh. 19 - Prob. 42PSCh. 19 - Which product, O2 or F2, is more likely to form at...Ch. 19 - Which product, Ca or H2, is more likely to form at...Ch. 19 - An aqueous solution of KBr is placed in a beaker...Ch. 19 - An aqueous solution of Na2S is placed in a beaker...Ch. 19 - In the electrolysis of a solution containing...Ch. 19 - In the electrolysis of a solution containing...Ch. 19 - Electrolysis of a solution of CuSO4(aq) to give...Ch. 19 - Electrolysis of a solution of Zn(NO3)2(aq) to give...Ch. 19 - A voltaic cell can be built using the reaction...Ch. 19 - Assume the specifications of a Ni-Cd voltaic cell...Ch. 19 - Prob. 53GQCh. 19 - Balance the following equations. (a) Zn(s) +...Ch. 19 - Magnesium metal is oxidized, and silver ions are...Ch. 19 - You want to set up a series of voltaic cells with...Ch. 19 - Prob. 57GQCh. 19 - Prob. 58GQCh. 19 - In the table of standard reduction potentials,...Ch. 19 - Prob. 60GQCh. 19 - Four voltaic cells are set up. In each, one...Ch. 19 - The following half-cells are available: (i)...Ch. 19 - Prob. 63GQCh. 19 - Prob. 64GQCh. 19 - A potential of 0.142 V is recorded (under standard...Ch. 19 - Prob. 66GQCh. 19 - The standard potential, E, for the reaction of...Ch. 19 - An electrolysis cell for aluminum production...Ch. 19 - Electrolysis of molten NaCl is done in cells...Ch. 19 - A current of 0.0100 A is passed through a solution...Ch. 19 - A current of 0.44 A is passed through a solution...Ch. 19 - Prob. 72GQCh. 19 - Prob. 73GQCh. 19 - Prob. 74GQCh. 19 - The products formed in the electrolysis of aqueous...Ch. 19 - Predict the products formed in the electrolysis of...Ch. 19 - Prob. 77GQCh. 19 - The metallurgy of aluminum involves electrolysis...Ch. 19 - Prob. 79GQCh. 19 - Prob. 80GQCh. 19 - Prob. 81GQCh. 19 - Prob. 82GQCh. 19 - Two Ag+(aq) | Ag(s) half-cells are constructed....Ch. 19 - Calculate equilibrium constants for the following...Ch. 19 - Prob. 85GQCh. 19 - Use the table of standard reduction potentials...Ch. 19 - Prob. 87GQCh. 19 - Prob. 88GQCh. 19 - Prob. 89GQCh. 19 - A voltaic cell is constructed in which one...Ch. 19 - An expensive but lighter alternative to the lead...Ch. 19 - The specifications for a lead storage battery...Ch. 19 - Manganese may play an important role in chemical...Ch. 19 - Prob. 94GQCh. 19 - Iron(II) ion undergoes a disproportionation...Ch. 19 - Copper(I) ion disproportionates to copper metal...Ch. 19 - Prob. 97GQCh. 19 - Prob. 98GQCh. 19 - Consider an electrochemical cell based on the...Ch. 19 - Prob. 100ILCh. 19 - A silver coulometer (Study Question 106) was used...Ch. 19 - Four metals, A, B, C, and D, exhibit the following...Ch. 19 - Prob. 103ILCh. 19 - The amount of oxygen, O2, dissolved in a water...Ch. 19 - Prob. 105SCQCh. 19 - The free energy change for a reaction, rG, is the...Ch. 19 - Prob. 107SCQCh. 19 - (a) Is it easier to reduce water in acid or base?...Ch. 19 - Prob. 109SCQ
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