Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 19, Problem 99IL

Consider an electrochemical cell based on the half-reactions Ni2+(aq) + 2 e → Ni(s) and Cd2+(aq) + 2e → Cd(s).

  1. (a) Diagram the cell, and label each of the components (including the anode, cathode, and salt bridge).
  2. (b) Use the equations for the half-reactions to write a balanced, net ionic equation for the overall cell reaction.
  3. (c) What is the polarity of each electrode?
  4. (d) What is the value of E°cell?
  5. (e) In which direction do electrons flow in the external circuit?
  6. (f) Assume that a salt bridge containing NaNO3 connects the two half-cells. In which direction do the Na+(aq) ions move? In which direction do the NO3 (aq) ions move?
  7. (g) Calculate the equilibrium constant for the reaction.
  8. (h) If the concentration of Cd2+ is reduced to 0.010 M and [Ni2+] = 1.0 M, what is the value of Ecell? Is the net reaction still the reaction given in part (b)?
  9. (i) If 0.050 A is drawn from the battery, how long can it last if you begin with 1.0 L of each of the solutions and each was initially 1.0 M in dissolved species? Each electrode weighs 50.0 g in the beginning.

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

The cell has to be drawn and label each of the component.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip  1

Explanation of Solution

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

The voltaic cell are as follows:

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip  2

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

The balance equation has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

Balanced reaction:Cd(s) + Ni2+(aq) Cd2+(aq) + Ni(s)

Explanation of Solution

Let’s write the half reactions occur at anode and cathode:

At anode:Cd(s) Cd2+(aq) + 2e-At cathode:Ni2+(aq)+2e- Ni(s)

By adding these two half reactions we get balanced reaction.

Cd(s) Cd2+(aq) + 2e-Ni2+(aq)+2e- Ni(s)________________________Cd(s) + Ni2+(aq) Cd2+(aq) + Ni(s)

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

The polarity of each electrode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

Anode is negative cathode is positive.

Explanation of Solution

In the voltaic cell has two voltaic cells. One electrode has positive charge called cathode and another electrode has negative called anode.

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

The Ecello has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

Ecello of the reaction is 0.15 V

Explanation of Solution

The reactions occur at anode and cathode is as follows.

At anode:Cd(s) Cd2+(aq) + 2e-    ; E0= -0.40 VAt cathode:Ni2+(aq)+2e- Ni(s)        ; E0= -0.25 V

Let’s calculate the Ecello of the reaction

Ecello=Ecathodeo-Eanodeo= -0.25 V-(-0.40) V= 0.15 V

 (e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

The direction in which electrons flow in the external circuit has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

Electrons are flow from anode to cathode.

Explanation of Solution

In the voltaic cell electrons are move anode to cathode.

(f)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

Assume that a salt bride containing NaNO3 connect the two half cells. It has to be identified in which direction do Na+(aq) ions and NO3- (aq) move.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

Na+ ions moves from anode to cathode

NO3- ions move from cathode to anode

Explanation of Solution

Salt bridge contains NaNO3 solution and it is dissociates into Na+ and NO3- ions.

Na+ ions moves from anode to cathode

NO3- ions move from cathode to anode

(g)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

The equilibrium constant has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

The equilibrium constant of the reaction is 1.1×105.

Explanation of Solution

lnK=nE00.0257=(2)(0.15 V)0.0257=11.673K=1.1 ×105

(h)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

If the concentration of Cd2+(aq) is reduced to 0.010 M and [Ni2+]=1.0 M. The Ecello of the reaction has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

Ecell of the reaction is 0.21 V.

Explanation of Solution

Ecell= Ecello-0.02572lnQ=Ecello-0.02572ln[Cd2+][Ni2+]=0.15 V-0.02572ln(0.010 M)(1.0 M)=0.21 V

Net reaction will be still given in part (b)

(i)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The half reactions are as follows.

Ni2+(aq) + 2e- Ni(s) and Cd2+(aq)+2e- Cd(s)

The time the battery will last if 0.050 M is drawn from the battery has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Answer to Problem 99IL

The time required for the electrolysis is 4800 h

Explanation of Solution

Moles of electrons required:Mole e-= (50 g Cd)(1 mol112.4 mol e-)(2 mol e-1 mol Cd)=0.88896 mol e-

Let’s calculate the charge of the cell:

Charge (C) = (0.8896 mol e-)(96500 C1 mol e-)= 8.58 u ×104 C

Therefore, the time can be calculated as follows.

Charge = Current (A) × time (s)8.584×104 C= 0.05 A ×time (s)time (s)=1.7×106 S=4800 h

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Chapter 19 Solutions

Chemistry & Chemical Reactivity

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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