Devise the electrochemical cell in which the cell reaction is Cu2+(aq.) + 2Cl-(aq.) + 2 Ag(s)  2 AgCl(s) + Cu(s) Write down the half-cell reactions for the corresponding electrodes, and the Nernst equation. Calculate the standard Gibbs free energy for the cell reaction, the equilibrium constant, and the standard potential of the cell from the thermodynamic data below Substance Cu2+(aq.) Cl-(aq.) AgCl(s)DfG0(kJ/mol) 65.5 -131 -110 c) Given that the standard potential of the Silver/Silver chloride electrode is 0.22V, calculate the standard potential of the Cu(s)/ Cu2+(aq.) electrode.

Answered: Image /qna-images/answer/9c0c7695-9fef-4249-8030-513c28fbf424.jpg

Answered: Devise the electrochemical cell in…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 14P

See similar textbooks

Related questions

Concept explainers

Question

Devise the electrochemical cell in which the cell reaction is

Cu²⁺(aq.) + 2Cl^-(aq.) + 2 Ag(s)  2 AgCl(s) + Cu(s)

Write down the half-cell reactions for the corresponding electrodes, and the Nernst equation.

Calculate the standard Gibbs free energy for the cell reaction, the equilibrium constant, and the standard potential of the cell from the thermodynamic data below

Substance Cu²⁺(aq.) Cl^-(aq.) AgCl(s)

D_fG⁰(kJ/mol) 65.5 -131 -110

c) Given that the standard potential of the Silver/Silver chloride electrode is 0.22V, calculate the standard potential of the Cu(s)/ Cu²⁺(aq.) electrode.

Expert Solution

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions