A voltaic cell is constructed with two silver–silver chloride electrodes, each of which is based on the following half-reaction:
AgCl(s) + e-→Ag(s) + Cl^-(aq)
The two half-cells have [Cl^-] = 0.0150 M and [Cl^-] = 2.55 M, respectively. (a) Which electrode is the cathode of the cell? (b) What is the standard emf of the cell? (c) What is the cell emf for the concentrations given? (d) For each electrode, predict whether [Cl^-] will increase, decrease, or stay the same as the cell operates.

Question

A voltaic cell is constructed with two silver–silver chloride electrodes, each of which is based on the following half-reaction:

AgCl(s) + e-→Ag(s) + Cl^-(aq)

The two half-cells have [Cl^-] = 0.0150 M and [Cl^-] = 2.55 M, respectively. (a) Which electrode is the cathode of the cell? (b) What is the standard emf of the cell? (c) What is the cell emf for the concentrations given? (d) For each electrode, predict whether [Cl^-] will increase, decrease, or stay the same as the cell operates.

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard