When [Hg2+] = 1.16 M, the observed cellpotential at 298 K for an electrochemicalcell with the reaction shown below is2.583 V. What is the Al3+ concentrationin this cell?3H92*(aq) + 2Al(s) – 3Hg(8) + 2AI3*(aq)[A|3*] =mol/L6.724x10^-4Show Approach Hide Tutor StepsResubmitTUTOR STEPThe first step is to separate the overallreaction into oxidation and reductionhalf-reactions. These are shown here.Hg2*(aq) + 2e" – Hg(e) reductionAl(s) → A3*(aq) + 3eoxidationNext(1 of 5)

Given, Ecell= 2.583V [Hg2+] = 1.16M

When [Hg2+] = 1.16 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 2.583 V. What is the Al3+ concentration in this cell? Знд2 (aq) + 2Al() — ЗHg(®) + 2A13*(aq)

When [Hg2+] = 1.16 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 2.583 V. What is the Al3+ concentration in this cell? Знд2 (aq) + 2Al() — ЗHg(®) + 2A13*(aq)

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 [Hg2+] = 1.16 M, the observed cell
potential at 298 K for an electrochemical
cell with the reaction shown below is
2.583 V. What is the Al3+ concentration
in this cell?
3H92*(aq) + 2Al(s) – 3Hg(8) + 2AI3*(aq)
[A|3*] =
mol/L
6.724x10^-4
Show Approach Hide Tutor Steps
Resubmit
TUTOR STEP
The first step is to separate the overall
reaction into oxidation and reduction
half-reactions. These are shown here.
Hg2*(aq) + 2e" – Hg(e) reduction
Al(s) → A3*(aq) + 3e
oxidation
Next
(1 of 5)

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