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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

Consider the following galvanic cell:

Chapter 18, Problem 151CP, Consider the following galvanic cell: Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the

Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is “dead.”

Interpretation Introduction

Interpretation:

The set up of a galvanic cell having Silver and Nickel electrode is given. The concentration of Ag+(aq) and Ni2+(aq) once the given cell is dead is to be calculated.

Concept introduction:

The equilibrium constant is used to determine the direction of the equilibrium. The higher value of K corresponds to the forward reaction and the lower value of K corresponds to the backward reaction.

To determine: The concentration of Ag+(aq) and Ni2+(aq) once the given cell is dead.

The value of K for the given cell reaction is 7.24×1034_ .

Explanation

The reaction taking place at the cathode is,

Ag++eAgE°red=0.80V

The reaction taking place at the anode is,

NiNi2++2eE°ox=0.23V

Multiply the reduction half-reaction with a coefficient of 2 and then add both the reduction and oxidation half-reactions as,

2Ag++2e2AgNiNi2++2e

The final equation is,

Ni+2Ag+2Ag+Ni2+

The value of E°cell is given as,

cell=E°ox+E°red

Where,

  • ox is the oxidation potential of the electrode.
  • red is the reduction potential of the electrode.

Substitute the values of E°ox and E°red in the above equation as,

cell=E°ox+E°red=0.23V+0.80V=1.03V

The cell potential is calculated using the Nernst equation,

E=E°-(0.0591n)log(Q)

Where,

  • E is the cell potential.
  • is the cell potential at the standard conditions.
  • Q is the activity of the species in the cell.
  • n is the number of electrons involved in the reaction.

As the cell is dead, it means the reaction has reached equilibrium. Therefore, at equilibrium, the value of Q is replaced with the equilibrium constant K and at equilibrium the value of E is equal to zero.

The reaction involves the transfer of 2 moles of electrons.

Rearrange the equation to obtain the value of E° as,

E°=E-(0.0591n)log(K)

Substitute the values of E , E° , n , in the above equation as,

E=E°-(0.0591n)log(K)0-1.03=-(0.05912)log(K)log(K)=34.86K=1034.86

The equation is further simplified as,

K=1034.86=7.24×1034_

The value of K for the given cell reaction is 7.24×1034_ .

The concentration of Ag+ from the reverse reaction is 0.46×10-17M_ and the concentration of Ni2+ from the reverse reaction is 1.5M_ .

The value of K for the given cell reaction is 7.24×1034_ .

As the value of equilibrium constant is high, it means that the reaction is about to complete.

Make the ICE table for the given cell reaction,

2Ag++Ni2Ag+Ni2+Initial:1

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Chapter 18 Solutions

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Ch-18 P-2ALQCh-18 P-3ALQCh-18 P-4ALQCh-18 P-5ALQCh-18 P-6ALQCh-18 P-7ALQCh-18 P-8ALQCh-18 P-9ALQCh-18 P-10ALQCh-18 P-11ALQCh-18 P-12ALQCh-18 P-13ALQCh-18 P-14ALQCh-18 P-15RORRCh-18 P-16RORRCh-18 P-17RORRCh-18 P-18RORRCh-18 P-19QCh-18 P-20QCh-18 P-21QCh-18 P-22QCh-18 P-23QCh-18 P-24QCh-18 P-25QCh-18 P-26QCh-18 P-27QCh-18 P-28QCh-18 P-29ECh-18 P-30ECh-18 P-31ECh-18 P-32ECh-18 P-33ECh-18 P-34ECh-18 P-35ECh-18 P-36ECh-18 P-37ECh-18 P-38ECh-18 P-39ECh-18 P-40ECh-18 P-41ECh-18 P-42ECh-18 P-43ECh-18 P-44ECh-18 P-45ECh-18 P-46ECh-18 P-47ECh-18 P-48ECh-18 P-49ECh-18 P-50ECh-18 P-51ECh-18 P-52ECh-18 P-53ECh-18 P-54ECh-18 P-55ECh-18 P-56ECh-18 P-57ECh-18 P-58ECh-18 P-59ECh-18 P-60ECh-18 P-61ECh-18 P-62ECh-18 P-63ECh-18 P-64ECh-18 P-65ECh-18 P-66ECh-18 P-68ECh-18 P-69ECh-18 P-70ECh-18 P-71ECh-18 P-72ECh-18 P-73ECh-18 P-74ECh-18 P-75ECh-18 P-76ECh-18 P-77ECh-18 P-78ECh-18 P-79ECh-18 P-80ECh-18 P-81ECh-18 P-82ECh-18 P-83ECh-18 P-84ECh-18 P-85ECh-18 P-86ECh-18 P-87ECh-18 P-88ECh-18 P-89ECh-18 P-90ECh-18 P-91ECh-18 P-92ECh-18 P-93ECh-18 P-94ECh-18 P-95ECh-18 P-96ECh-18 P-97ECh-18 P-98ECh-18 P-99ECh-18 P-100ECh-18 P-101ECh-18 P-102ECh-18 P-103ECh-18 P-104ECh-18 P-105ECh-18 P-106ECh-18 P-107ECh-18 P-108ECh-18 P-109ECh-18 P-110ECh-18 P-111ECh-18 P-112ECh-18 P-113AECh-18 P-114AECh-18 P-115AECh-18 P-116AECh-18 P-117AECh-18 P-118AECh-18 P-119AECh-18 P-120AECh-18 P-121AECh-18 P-122AECh-18 P-123AECh-18 P-124AECh-18 P-125AECh-18 P-126AECh-18 P-127AECh-18 P-128AECh-18 P-129AECh-18 P-130AECh-18 P-131AECh-18 P-132AECh-18 P-133AECh-18 P-134CWPCh-18 P-135CWPCh-18 P-136CWPCh-18 P-137CWPCh-18 P-138CWPCh-18 P-139CWPCh-18 P-140CPCh-18 P-141CPCh-18 P-142CPCh-18 P-143CPCh-18 P-144CPCh-18 P-145CPCh-18 P-146CPCh-18 P-147CPCh-18 P-148CPCh-18 P-149CPCh-18 P-150CPCh-18 P-151CPCh-18 P-152CPCh-18 P-153CPCh-18 P-154CPCh-18 P-155IPCh-18 P-156IPCh-18 P-157IPCh-18 P-158IPCh-18 P-159MPCh-18 P-160MP

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