Ch.18 - ElectrochemistryWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: 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 cell compartments have [Cl- ]

Solution: 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 cell compartments have [Cl- ]

Problem

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 cell compartments have [Cl- ] = 1.51×10−2 M and [Cl- ] = 2.60 M , respectively.

For the cathode compartment, predict whether [Cl- ] will increase, decrease, or stay the same as the cell operates.

Solution

We are asked to determine if the [Cl-] will increase, decrease or stay the same in the cathode department in the voltaic cell given.


We have to determine the anode (oxidation) and cathode (reduction) reactions in the concentration cell.

View the complete written solution...