An electrochemical cell is given with a cell reaction of Pb²⁺ + Cd → Pb + Cd²⁺ at 25°C with ion concentrations of [Cd²⁺] = 2 M, and [Pb²⁺] = 1.49×10⁻⁹ M. Used the photo as a reference.1. What can be said of the reaction at the specified concentration of ions?2. What is the equilibrium constant for the reaction? Use R = 8.31447 J/mol K and F = 96,485 C/mol e-.Standard reduction potentials for some common metals - for aqueoussolutions of ions at 1.0 M concentration at 25 °C and H2 gas at 1.0 atmpressure and 25°CReduction Half-Cell EquationLi+ + 1e →→→ LiK+ + 1e-→ KBa2+ + 2e → BaCa2+ + 2e → CaNa + 1e O NaMg2+ + 2e→→ MgAl3+ + 3e → AlZn2+ + 2e- → ZnCr³+ + 3e → CrFe2+ + 2e→ FeCd²+ + 2e-Ni2+ + 2eSn²+ + 2esnPb2+ + 2e → Pb→ Cd→ Ni2 H+ + 2e → H2Cu2+ + 2e→ CuHg2+ + 2e → 2 HgAg+ +1eAgHg2+ + 2e →→ HgAu³+ + 3e → AuE° (v)-3.04-2.92-2.91-2.87-2.71-2.36-1.66-0.76-0.74-0.44-0.40-0.25-0.14-0.130.00+0.34+0.79+0.80+0.85+1.42

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Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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An electrochemical cell is given with a cell reaction of Pb²⁺ + Cd → Pb + Cd²⁺ at 25°C with ion concentrations of [Cd²⁺] = 2 M, and [Pb²⁺] = 1.49×10⁻⁹ M. Used the photo as a reference.

1. What can be said of the reaction at the specified concentration of ions?
2. What is the equilibrium constant for the reaction?

Use R = 8.31447 J/mol K and F = 96,485 C/mol e-.
Standard reduction potentials for some common metals - for aqueous
solutions of ions at 1.0 M concentration at 25 °C and H2 gas at 1.0 atm
pressure and 25°C
Reduction Half-Cell Equation
Li+ + 1e →→→ Li
K+ + 1e-
→ K
Ba2+ + 2e → Ba
Ca2+ + 2e → Ca
Na + 1e O Na
Mg2+ + 2e
→→ Mg
Al3+ + 3e → Al
Zn2+ + 2e- → Zn
Cr³+ + 3e → Cr
Fe2+ + 2e
→ Fe
Cd²+ + 2e-
Ni2+ + 2e
Sn²+ + 2e
sn
Pb2+ + 2e → Pb
→ Cd
→ Ni
2 H+ + 2e → H2
Cu2+ + 2e
→ Cu
Hg2+ + 2e → 2 Hg
Ag+ +1e
Ag
Hg2+ + 2e →→ Hg
Au³+ + 3e → Au
E° (v)
-3.04
-2.92
-2.91
-2.87
-2.71
-2.36
-1.66
-0.76
-0.74
-0.44
-0.40
-0.25
-0.14
-0.13
0.00
+0.34
+0.79
+0.80
+0.85
+1.42

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