Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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Chapter 17, Problem 107QRT

(a)

Interpretation Introduction

Interpretation:

The cell potential at standard conditions has to be calculated.

Concept Introduction:

The cell potential is defined as the potential difference that gets created between the electrodes of a cell due to the movement of electrons from anode to the cathode.  The unit of cell potential is volts.  An electrochemical cell is used to produce electricity by converting the chemical energy which is produced by the reactions occurring in a cell.  It consists of a cathode for the reduction reaction and anode for the oxidation reaction.

(a)

Expert Solution
Check Mark

Answer to Problem 107QRT

The cell potential at standard conditions is 0.127V_.

Explanation of Solution

The E° value of Cr2+|Cr is 0.89V.

The E° value of Zn2+|Zn is 0.763V.

The E° value of Zn2+ is higher than that of Cr2+.

Therefore, in the given voltaic cell Zn2+ will undergo reduction at cathode and Cr2+ will undergoes oxidation at anode.

The oxidation half-reaction at anode is shown below.

    Cr(s)Cr2+(aq)+2e

The reduction half-reaction at cathode is shown below.

    Zn2+(aq)+2eZn(s)

The overall reaction is obtained by adding oxidation half-reaction and reduction-half reaction as shown below.

    Cr(s)Cr2+(aq)+2eZn2+(aq)+2eZn(s)

    Zn2+(aq)+Cr(s)Zn(s)+Cr2+(aq)¯

The formula to calculate standard cell potential of the above reaction is shown below.

    Ecellο=EcathodeοEanodeο

Where,

  • Ecathodeο is the electrode potential of cathode.
  • Eanodeο is the electrode potential of anode.
  • Ecellο is the standard cell potential.

The value of Ecathodeο is 0.763V

The value of Eanodeο is 0.89V

Substitute the values of Eanodeο and Ecathodeο in the above formula.

  Ecellο=EcathodeοEanodeο=0.763V(0.89V)=0.127V

Therefore, the value of standard cell potential is 0.127V_.

(b)

Interpretation Introduction

Interpretation:

The value of Gibbs’s energy change ΔrGcellο has to be calculated.

Concept Introduction:

Refer to part (a).

(b)

Expert Solution
Check Mark

Answer to Problem 107QRT

The value of ΔrGcellο is -24507.19J_.

Explanation of Solution

The formula to calculate ΔrGcellο of the cell is given below.

    ΔrGcellο=nFEcellο

Where,

  • n is the number of electrons exchanged within the cell.
  • F is the Faraday’s constant.
  • Ecellο is the standard cell potential of the cell.

The value of n is 2.

The value of F is 96485C/mol.

The value of Ecellο is 0.127V.

Substitute the values of n, F and Ecellο in the formula to calculate the value of ΔrGcellο.

  ΔrGcellο=nFEcellοΔrGcellο=2×96485C/mol×0.127V=24507.19J

Therefore, the value of ΔrGcellο is -24507.19J_.

(c)

Interpretation Introduction

Interpretation:

The value of ΔrGcell and Ecell has to be calculated.

Concept Introduction:

Refer to part (a).

(c)

Expert Solution
Check Mark

Answer to Problem 107QRT

The value the cell potential of the cell is -0.058V_.

The value of ΔrGcell is 11192.26J_.

Explanation of Solution

The concentration of Zn2+ is 0.010V.

The concentration of Cr2+ is 0.050V.

The formula to calculate Ecell for the given cell is shown below.

    Ecell=Ecellο0.529nlog[Cr2+][Zn2+]

Where,

  • Ecellο is the standard cell potential of the cell.
  • n is the number of electrons transferred in the cell.
  • [Cr2+] is the concentration of Cr2+.
  • [Zn2+] is the concentration of Zn2+.

The value of n is 2.

The value of Ecellο is 0.127V.

The value of [Cr2+] is 0.050M.

The value of [Zn2+] is 0.010V.

Substitute the values of n, Ecellο, [Cr2+] and [Zn2+] in the formula.

    Ecell=Ecellο0.529nlog[Cr2+][Zn2+]Ecell=0.127V0.5292log(0.050M0.010M)=0.127V0.2645×log(5)=0.127V0.2645×(0.69897)

On further solving the equation,

    Ecell=0.127V0.2645×(0.69897)=0.127V0.185=0.058V

Therefore, the cell potential of the cell is -0.058V_.

The formula to calculate ΔrGcell of the cell is given below.

    ΔrGcell=nFEcell

Where,

  • n is the number of electrons exchanged within the cell.
  • F is the Faraday’s constant.
  • Ecell is the standard cell potential of the cell.

The value of n is 2.

The value of F is 96485C/mol.

The value of Ecell is 0.058V

Substitute the values of n, F and Ecell in the formula to calculate the value of ΔrGcell.

  ΔrGcell=nFEcellΔrGcell=2×96485C/mol×(0.058V)=11192.26J

Therefore, the value of ΔrGcell is 11192.26J_.

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Chapter 17 Solutions

Chemistry: The Molecular Science

Ch. 17.4 - Given this reaction, its standard potential, and...Ch. 17.5 - Prob. 17.5PSPCh. 17.5 - Prob. 17.8CECh. 17.5 - Prob. 17.9CECh. 17.5 - Prob. 17.10CECh. 17.6 - Prob. 17.6PSPCh. 17.6 - Prob. 17.11ECh. 17.6 - Prob. 17.7PSPCh. 17.7 - Calculate the cell potential for the Zn(s) +...Ch. 17.7 - Prob. 17.9PSPCh. 17.8 - Prob. 17.12ECh. 17.8 - Prob. 17.13ECh. 17.8 - Prob. 17.14ECh. 17.10 - Predict the results of passing a direct electrical...Ch. 17.10 - In 1886. Henri Moissan was the first to prepare...Ch. 17.11 - In the commercial production of sodium metal by...Ch. 17.11 - Prob. 17.16CECh. 17.11 - Prob. 17.17ECh. 17.11 - Prob. 17.18CECh. 17.11 - Prob. 17.19ECh. 17.12 - Prob. 17.20CECh. 17.12 - Prob. 17.21CECh. 17 - Prob. 2SPCh. 17 - Prob. 1QRTCh. 17 - Prob. 2QRTCh. 17 - Prob. 3QRTCh. 17 - Prob. 4QRTCh. 17 - Identify each statement as true or false. Rewrite...Ch. 17 - Prob. 6QRTCh. 17 - Prob. 7QRTCh. 17 - Prob. 8QRTCh. 17 - Answer Question 8 again, but this time find a...Ch. 17 - Prob. 10QRTCh. 17 - Prob. 11QRTCh. 17 - For the reaction in Question 6, write balanced...Ch. 17 - Prob. 13QRTCh. 17 - Prob. 14QRTCh. 17 - Prob. 15QRTCh. 17 - Prob. 16QRTCh. 17 - Prob. 17QRTCh. 17 - For the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+...Ch. 17 - Prob. 19QRTCh. 17 - Prob. 20QRTCh. 17 - Prob. 21QRTCh. 17 - Prob. 22QRTCh. 17 - Draw a diagram of each cell. Label the anode, the...Ch. 17 - Prob. 24QRTCh. 17 - Prob. 25QRTCh. 17 - Prob. 26QRTCh. 17 - Prob. 27QRTCh. 17 - Prob. 28QRTCh. 17 - Prob. 29QRTCh. 17 - Prob. 30QRTCh. 17 - Prob. 31QRTCh. 17 - Consider these half-reactions: (a) Which is the...Ch. 17 - Consider these half-reactions: (a) Which is the...Ch. 17 - In principle, a battery could be made from...Ch. 17 - Prob. 35QRTCh. 17 - Hydrazine, N2H4, can be used as the reducing agent...Ch. 17 - Prob. 37QRTCh. 17 - Prob. 38QRTCh. 17 - Prob. 39QRTCh. 17 - Prob. 40QRTCh. 17 - Prob. 41QRTCh. 17 - Prob. 42QRTCh. 17 - Prob. 43QRTCh. 17 - Prob. 44QRTCh. 17 - Prob. 45QRTCh. 17 - Prob. 46QRTCh. 17 - Consider the voltaic cell 2 Ag+(aq) + Cd(s) 2...Ch. 17 - Consider a voltaic cell with the reaction H2(g) +...Ch. 17 - Calculate the cell potential of a concentration...Ch. 17 - Prob. 50QRTCh. 17 - Prob. 51QRTCh. 17 - Prob. 52QRTCh. 17 - Prob. 53QRTCh. 17 - NiCad batteries are rechargeable and are commonly...Ch. 17 - Prob. 55QRTCh. 17 - Prob. 56QRTCh. 17 - Prob. 57QRTCh. 17 - Hydrazine, N2H4, has been proposed as the fuel in...Ch. 17 - Consider the electrolysis of water in the presence...Ch. 17 - Prob. 60QRTCh. 17 - Prob. 61QRTCh. 17 - Prob. 62QRTCh. 17 - Identify the products of the electrolysis of a 1-M...Ch. 17 - Prob. 64QRTCh. 17 - Prob. 65QRTCh. 17 - Prob. 66QRTCh. 17 - Prob. 67QRTCh. 17 - Prob. 68QRTCh. 17 - Prob. 69QRTCh. 17 - Prob. 70QRTCh. 17 - Prob. 71QRTCh. 17 - Prob. 72QRTCh. 17 - Prob. 73QRTCh. 17 - Prob. 74QRTCh. 17 - Calculate how long it would take to electroplate a...Ch. 17 - Prob. 76QRTCh. 17 - Prob. 77QRTCh. 17 - Prob. 78QRTCh. 17 - Prob. 79QRTCh. 17 - Prob. 80QRTCh. 17 - Prob. 81QRTCh. 17 - Prob. 82QRTCh. 17 - Prob. 83QRTCh. 17 - Prob. 84QRTCh. 17 - Prob. 85QRTCh. 17 - Prob. 86QRTCh. 17 - Prob. 87QRTCh. 17 - Prob. 88QRTCh. 17 - You wish to electroplate a copper surface having...Ch. 17 - Prob. 90QRTCh. 17 - Prob. 91QRTCh. 17 - Prob. 92QRTCh. 17 - Prob. 93QRTCh. 17 - An electrolytic cell is set up with Cd(s) in...Ch. 17 - Prob. 95QRTCh. 17 - Prob. 96QRTCh. 17 - Prob. 97QRTCh. 17 - Prob. 98QRTCh. 17 - Prob. 99QRTCh. 17 - Prob. 100QRTCh. 17 - Prob. 101QRTCh. 17 - Prob. 102QRTCh. 17 - Prob. 103QRTCh. 17 - Prob. 104QRTCh. 17 - Prob. 105QRTCh. 17 - Prob. 106QRTCh. 17 - Prob. 107QRTCh. 17 - Prob. 108QRTCh. 17 - Prob. 109QRTCh. 17 - Prob. 110QRTCh. 17 - Prob. 111QRTCh. 17 - Prob. 17.ACPCh. 17 - Prob. 17.BCP
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