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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?

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?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section17.4: Voltaic Cells And Cell Potential
Problem 17.4PSP: Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the...
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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
Transcribed Image Text: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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