General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN: 9781305580343
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher: Cengage Learning
Question
Chapter 19, Problem 19.146QP

 (a)

Interpretation Introduction

Interpretation:

The cell potential (EMF) of given cell should be calculated at standard conditions by using Nernst equation.

Concept introduction:

Cell potential (EMF):

The maximum potential difference between two electrodes of voltaic cell is known as cell potential.

If standard reduction potentials of electrodes are given the cell potential (EMF) is given by,

Ecell=Ecathode-Eanode

Where,

Ecathodeisthereductionhalfcell potentialEanodeistheoxidationhalfcell potential

Nernst equation:

The relationship between standard cell potential and cell potential at non standard conditions and the reaction quotient are given by Nernst equation it is,

Ecell=cell-2.303RTnFlogQ

Where,

Ecell iscell potentialcellisstandard cell potentialRisgasconstantTistemperatureQisreaction quotient

 (a)

Expert Solution
Check Mark

Answer to Problem 19.146QP

The cell potential (EMF) of given voltaic cell is 1.56V

Explanation of Solution

To calculate the cell potential (EMF) of given cell

The standard reduction potentials of (SRP) of Zinc and Silver are record from standard reduction potentials table and they are,

Zn(s)Zn2+(aq)+2e--=0.76V2Ag+(aq)+2e-2Ag(s)E°=0.80V

The most positive SQR is considering as cathode potential.

The SRP of electrodes are plugged in the bellow equation to give cell potential of given voltaic cell.

Ecell=Ecathode-Eanode=0.80-(-0.76)=1.56V

The cell potential (EMF) of given voltaic cell is 1.56V

To calculate the cell potential (EMF) of given cell

Given:

Mass of ZnNO3 is 105g

Mass of AgNO3 is 145g

Final volume of ZnNO3 solution is 1.1L

Final volume of AgNO3 solution is 1 L

To calculate the concentrations of ZnNO3 and AgNO3 solutions

Molar mass of AgNO3 is 169.99g

[Ag+]=145gAgNO31.0L×1molAgNO3169.99gAgNO3×1molAg+1molAgNO3=0.854MAg+

Molar mass of ZnNO3 is 189.40g

[Zn2+]=105gZnNO31.1L×1molZnNO3189.40gZnNO3×1molZn2+1molZnNO3=0.504MZn2+

Taken mass and molar mass of ZnNO3 , AgNO3 and volumes of solutions are plugged in above equations to give concentrations of Zn2+ and Ag+ ions.

In this cell reaction, number of electrons transferred are 2

Faraday constant is 96485C mol1

Ecell=cell-2.303RTnFlogQ=cell0.0592nlogQWeknow,Q=productsreactants=1.56V-0.05922log[Zn2+][Ag+]2=1.56V-0.05922log[0.504][0.854]2=1.56V-(-0.00475V)=1.56475V=1.56V

The calculated standard cell potential (EMF) of given voltaic cell, number of electron transferred in cell reaction, Faraday constant and calculated concentrations of ions are plugged in the above equation to give a cell potential (EMF) of given cell at non standard conditions.

The cell potential (EMF) of given cell at non-standard conditions is 1.56V

Conclusion

The cell potential (EMF) of given cell was calculated at standard condition by using Nernst equation and it was found to be 1.56V

(b)

Interpretation Introduction

Interpretation:

The free energy change of given voltaic cell should be calculated by using standard reduction potentials and cell potential of the cell should be explained, when doing given operations to the cell.

Concept introduction:

Free energy change:

In thermodynamics the cell potential is known as  maximum work of the cell and it is equal to free energy change of the cell and it is given by,

ΔG=-nFEcell

Where,

ΔGisfreeenergychangenisnumberofelectrontransferredFisfaraday constantEcelliscell potential

(b)

Expert Solution
Check Mark

Answer to Problem 19.146QP

Solution:

The free energy change of voltaic cell is -301.0KJ

Explanation of Solution

To calculate the free energy change of given cell:

In this cell reaction number of electron transferred are 2

Faraday constant is 96485C mol1

ΔG=-nFEcell=-2mole×96485Cmole-1×1.56V=-3.010×105CV=-3.010×105J=-301.0KJ

The calculated cell potential (EMF) of given voltaic cell and number of electron transferred in cell reaction and Faraday constant are plugged in the above equation to give a free energy change of given cell.

The free energy change of given cell reaction is -301.0KJ

(c)

Interpretation Introduction

Interpretation:

The cell potential (EMF) of given cell should be explained in terms of concentration of AgNO3 solution.

Concept introduction:

Nernst equation:

The relationship between standard cell potential and cell potential at standard conditions and the reaction quotient are given by Nernst equation it is,

Ecell=cell-2.303RTnFlogQ

Where,

Ecell iscell potentialcellisstandard cell potentialRisgasconstantTistemperatureQisreaction quotient

(c)

Expert Solution
Check Mark

Answer to Problem 19.146QP

The concentration of Ag+ is same therefore the cell potential is remains same and it is 1.56V

Explanation of Solution

According to the Nernst equation, the concentration of makes changes in cell potential but in addition of 25.0 mL AgNO3 is also being a same concentration so there is no concentration changes offered, when addition of 25.0 mL AgNO3 .

Hence, the concentration of Ag+ is same therefore the cell potential is remains same and it is 1.56V

(d)

Interpretation Introduction

Interpretation:

The cell potential (EMF) of given cell should be explained in terms of electrode concentration.

Concept introduction:

Nernst equation:

The relationship between standard cell potential and cell potential at standard conditions and the reaction quotient are given by Nernst equation it is,

Ecell=cell-2.303RTnFlogQ

Where,

Ecell iscell potentialcellisstandard cell potentialRisgasconstantTistemperatureQisreaction quotient

(d)

Expert Solution
Check Mark

Answer to Problem 19.146QP

The cell potential would not affected by increasing mass of zinc electrode.

Explanation of Solution

The cell potential does not depended on mass of electrodes in voltaic cell.

Hence, the cell potential would not affected by increasing mass of zinc electrode.

(e)

Interpretation Introduction

Interpretation:

The cell potential (EMF) of given cell should be explained, when the addition of NaCl into AgNO3 half cell.

Concept introduction:

Nernst equation:

The relationship between standard cell potential and cell potential at standard conditions and the reaction quotient are given by Nernst equation it is,

Ecell=cell-2.303RTnFlogQ

Where,

Ecell iscell potentialcellisstandard cell potentialRisgasconstantTistemperatureQisreaction quotient

(e)

Expert Solution
Check Mark

Answer to Problem 19.146QP

The addition of NaCl is decreases the cell potential of give cell.

Explanation of Solution

According to the Nernst equation, the addition of NaCl into AgNO3 half cell will causes AgCl to precipitated, result of this the concentration of Ag+ ion is decreases, in order reaction quotient value also decreases.

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Chapter 19 Solutions

General Chemistry - Standalone book (MindTap Course List)

Ch. 19.5 - Prob. 19.2CCCh. 19.6 - Prob. 19.10ECh. 19.6 - Prob. 19.11ECh. 19.6 - Prob. 19.12ECh. 19.7 - What is the cell potential of the following...Ch. 19.7 - What is the nickel(II)-ion concentration in the...Ch. 19.7 - Prob. 19.3CCCh. 19.8 - Prob. 19.4CCCh. 19.9 - Write the half-reactions for the electrolysis of...Ch. 19.10 - Prob. 19.16ECh. 19.11 - A constant electric current deposits 365 mg of...Ch. 19.11 - How many grams of oxygen are liberated by the...Ch. 19 - Describe the difference between a voltaic cell and...Ch. 19 - Prob. 19.2QPCh. 19 - What is the SI unit of electrical potential?Ch. 19 - Define the faraday.Ch. 19 - Why is it necessary to measure the voltage of a...Ch. 19 - Prob. 19.6QPCh. 19 - Prob. 19.7QPCh. 19 - Prob. 19.8QPCh. 19 - Prob. 19.9QPCh. 19 - Prob. 19.10QPCh. 19 - Prob. 19.11QPCh. 19 - Prob. 19.12QPCh. 19 - Prob. 19.13QPCh. 19 - Prob. 19.14QPCh. 19 - Prob. 19.15QPCh. 19 - Prob. 19.16QPCh. 19 - Briefly explain why different products are...Ch. 19 - Prob. 19.18QPCh. 19 - Prob. 19.19QPCh. 19 - What half-reaction would be expected to occur at...Ch. 19 - Prob. 19.21QPCh. 19 - The voltaic cell is represented as...Ch. 19 - Electrochemical Cells I You have the following...Ch. 19 - Electrochemical Cells II Consider this cell...Ch. 19 - Prob. 19.25QPCh. 19 - Prob. 19.26QPCh. 19 - Prob. 19.27QPCh. 19 - Prob. 19.28QPCh. 19 - Prob. 19.29QPCh. 19 - Prob. 19.30QPCh. 19 - Prob. 19.31QPCh. 19 - You have 1.0 M solutions of Al(NO3)3 and AgNO3...Ch. 19 - The zinc copper voltaic cell shown with this...Ch. 19 - The development of lightweight batteries is an...Ch. 19 - Prob. 19.35QPCh. 19 - Prob. 19.36QPCh. 19 - Balance the following oxidationreduction...Ch. 19 - Balance the following oxidationreduction...Ch. 19 - Balance the following oxidationreduction...Ch. 19 - Prob. 19.40QPCh. 19 - Balance the following oxidationreduction...Ch. 19 - Prob. 19.42QPCh. 19 - A voltaic cell is constructed from the following...Ch. 19 - Half-cells were made from a nickel rod dipping in...Ch. 19 - Zinc react spontaneously with silver ion....Ch. 19 - Prob. 19.46QPCh. 19 - A silver oxidezinc cell maintains a fairly...Ch. 19 - A mercury battery, used for hearing aids and...Ch. 19 - Write the cell notation for a voltaic cell with...Ch. 19 - Write the cell notation for a voltaic cell with...Ch. 19 - Give the notation for a voltaic cell constructed...Ch. 19 - A voltaic cell has an iron rod in 0.30 M iron(III)...Ch. 19 - Prob. 19.53QPCh. 19 - Write the overall cell reaction for the following...Ch. 19 - Consider the voltaic cell...Ch. 19 - Consider the voltaic cell...Ch. 19 - A voltaic cell whose cell reaction is...Ch. 19 - A particular voltaic cell operates on the reaction...Ch. 19 - What is the maximum work you can obtain from 30.0...Ch. 19 - Calculate the maximum work available from 50.0 g...Ch. 19 - Order the following oxidizing agents by increasing...Ch. 19 - Order the following oxidizing agents by increasing...Ch. 19 - Consider the reducing agents Cu+(aq), Zn(s), and...Ch. 19 - Prob. 19.64QPCh. 19 - Prob. 19.65QPCh. 19 - Answer the following questions by referring to...Ch. 19 - Prob. 19.67QPCh. 19 - Dichromate ion, Cr2O72, is added to an acidic...Ch. 19 - Calculate the standard cell potential of the...Ch. 19 - Calculate the standard cell potential of the...Ch. 19 - What is the standard cell potential you would...Ch. 19 - What is the standard cell potential you would...Ch. 19 - Calculate the standard free-energy change at 25C...Ch. 19 - Calculate the standard free-energy change at 25C...Ch. 19 - What is G for the following reaction?...Ch. 19 - Prob. 19.76QPCh. 19 - Calculate the standard cell potential at 25C for...Ch. 19 - Calculate the standard cell potential at 25C for...Ch. 19 - Prob. 19.79QPCh. 19 - Calculate the standard cell potential of the cell...Ch. 19 - Calculate the equilibrium constant K for the...Ch. 19 - Calculate the equilibrium constant K for the...Ch. 19 - Copper(I) ion can act as both an oxidizing agent...Ch. 19 - Prob. 19.84QPCh. 19 - Calculate the cell potential of the following cell...Ch. 19 - What is the cell potential of the following cell...Ch. 19 - Calculate the cell potential of a cell operating...Ch. 19 - Calculate the cell potential of a cell operating...Ch. 19 - The voltaic cell Cd(s)Cd2+(aq)Ni2+(1.0M)Ni(s) has...Ch. 19 - The cell potential of the following cell at 25C is...Ch. 19 - What are the half-reactions in the electrolysis of...Ch. 19 - What are the half-reactions in the electrolysis of...Ch. 19 - Describe what you expect to happen when the...Ch. 19 - Prob. 19.94QPCh. 19 - In the commercial preparation of aluminum,...Ch. 19 - Chlorine, Cl2, is produced commercially by the...Ch. 19 - When molten lithium chloride, LiCl, is...Ch. 19 - How many grams of cadmium are deposited from an...Ch. 19 - Some metals, such as iron, can be oxidized to more...Ch. 19 - Some metals, such as thallium, can be oxidized to...Ch. 19 - Balance the following skeleton equations. The...Ch. 19 - Prob. 19.102QPCh. 19 - Prob. 19.103QPCh. 19 - Prob. 19.104QPCh. 19 - Prob. 19.105QPCh. 19 - Give the notation for a voltaic cell whose overall...Ch. 19 - Prob. 19.107QPCh. 19 - Use electrode potentials to answer the following...Ch. 19 - Prob. 19.109QPCh. 19 - Prob. 19.110QPCh. 19 - a Calculate the equilibrium constant for the...Ch. 19 - Prob. 19.112QPCh. 19 - How many faradays are required for each of the...Ch. 19 - Prob. 19.114QPCh. 19 - In an analytical determination of arsenic, a...Ch. 19 - Prob. 19.116QPCh. 19 - Prob. 19.117QPCh. 19 - Prob. 19.118QPCh. 19 - A solution of copper(II) sulfate is electrolyzed...Ch. 19 - A potassium chloride solution is electrolyzed by...Ch. 19 - A constant current of 1.40 amp is passed through...Ch. 19 - A constant current of 1.25 amp is passed through...Ch. 19 - An aqueous solution of an unknown salt of gold is...Ch. 19 - An aqueous solution of an unknown salt of vanadium...Ch. 19 - An electrochemical cell is made by placing a zinc...Ch. 19 - An electrochemical cell is made by placing an iron...Ch. 19 - Prob. 19.127QPCh. 19 - a Calculate G for the following cell reaction:...Ch. 19 - Prob. 19.129QPCh. 19 - Prob. 19.130QPCh. 19 - A voltaic cell is constructed from a half-cell in...Ch. 19 - Prob. 19.132QPCh. 19 - Prob. 19.133QPCh. 19 - Order the following oxidizing agents by increasing...Ch. 19 - What is the cell potential (Ecell) of a...Ch. 19 - Prob. 19.136QPCh. 19 - Which of the following reactions occur...Ch. 19 - Prob. 19.138QPCh. 19 - The following two half-reactions arc involved in a...Ch. 19 - Prob. 19.140QPCh. 19 - Prob. 19.141QPCh. 19 - A 1.0-L sample of 1.0 M HCl solution has a 10.0 A...Ch. 19 - Consider the following cell running under standard...Ch. 19 - Prob. 19.144QPCh. 19 - Prob. 19.145QPCh. 19 - Prob. 19.146QPCh. 19 - Consider the following cell reaction at 25C....Ch. 19 - Consider the following cell reaction at 25C....Ch. 19 - Prob. 19.149QPCh. 19 - Prob. 19.150QPCh. 19 - Prob. 19.151QPCh. 19 - Prob. 19.152QPCh. 19 - An electrode is prepared by dipping a silver strip...Ch. 19 - An electrode is prepared from liquid mercury in...
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