When [Pb2+] = 1.40 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 1.150 V. What is the Mn2+ concentration in thiscell?Pb2*(aq) + Mn(s)– Pb(s) + Mn²+(aq)[Mn2+] =mol/L Step 1Decompose the cell reaction given into half-cell reactions and look up the standard electrode potentials.Step 2Use these to calculate the standard cell potential: E°cell = E°cathode - E°anodeStep 3Determine the value of the reaction quotient, Q, using the value of E° cell and the measured value of Ecel-At 298 K,Ecel = Eel0.0257 VIn QStep 4Calculate the unknown concentration using the values of Q and the known concentrations.

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When [Pb2+] = 1.40 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 1.150 V. What is the Mn2+ concentration in this cell? Pb2*(aq) + Mn(s)– Pb(s) + Mn²+(aq) [Mn2+] = mol/L

When [Pb2+] = 1.40 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 1.150 V. What is the Mn2+ concentration in this cell? Pb2*(aq) + Mn(s)– Pb(s) + Mn²+(aq) [Mn2+] = mol/L

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

When [Pb2+] = 1.40 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 1.150 V. What is the Mn2+ concentration in this
cell?
Pb2*(aq) + Mn(s)– Pb(s) + Mn²+(aq)
[Mn2+] =
mol/L

Step 1
Decompose the cell reaction given into half-cell reactions and look up the standard electrode potentials.
Step 2
Use these to calculate the standard cell potential: E°cell = E°cathode - E°anode
Step 3
Determine the value of the reaction quotient, Q, using the value of E° cell and the measured value of Ecel-
At 298 K,
Ecel = Eel
0.0257 V
In Q
Step 4
Calculate the unknown concentration using the values of Q and the known concentrations.

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