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:
Corrosion of iron in contact with water. One region of the iron acts as the cathode and another region acts as the anode.
What is the oxidizing agent in this corrosion reaction?

Solution: Corrosion of iron in contact with water. One region of the iron acts as the cathode and another region acts as the anode.What is the oxidizing agent in this corrosion reaction?

Problem

A diagram shows a piece of solid iron with a water drop on top. 1. Fe is oxidized at the anode region of the metal.  Fe goes to Fe2+ plus 2 e-. 2. Electrons from Fe oxidation migrate to the region acting as the cathode. 3. O2 is reduced at the cathode region.  O2 plus 4 H+ plus 4 e- goes to 2 H2O, or O2 plus 2 H2O plus 4 e- goes to 4 OH-. 4. Fe2+ is oxidized to Fe3+ as rust (Fe2O3) forms.
Corrosion of iron in contact with water. One region of the iron acts as the cathode and another region acts as the anode.

What is the oxidizing agent in this corrosion reaction?