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 based on Ag+(aq)/Ag(s) and Fe3+(aq)/Fe2+(aq) half-cells.Which reaction occurs at the cathode, and which at the anode of the cell?

Solution: A voltaic cell is based on Ag+(aq)/Ag(s) and Fe3+(aq)/Fe2+(aq) half-cells.Which reaction occurs at the cathode, and which at the anode of the cell?

Problem

A voltaic cell is based on Ag+(aq)/Ag(s) and Fe3+(aq)/Fe2+(aq) half-cells.

Which reaction occurs at the cathode, and which at the anode of the cell?

Solution

We are being asked to determine which reaction occurs at the cathode and which reaction occurs at the anode for a voltaic cell.

Recall:voltaic cell represents an electrochemical cell that is spontaneous

It has two half-cells, specifically, the anode and the cathode.

Each cell has a cell potential expressed by E or E°. (E° is the cell potential at standard conditions)

The greater the cell potential then the more likely reduction occurs. The smaller the cell potential then the more likely oxidation occurs. Reduction occurs at the cathode and oxidation occurs at the anode.


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