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: Determine the redox reaction represented by the following cell notation. Fe(s) | Fe2+(aq) ‖ Cu2+(aq) | Cu(s)   a) Cu(s) + Fe2+(aq) → Fe(s) + Cu 2+(aq) b) Fe(s) + Cu2+(aq) → Cu(s) + Fe 2+(aq) c) 2

Problem

Determine the redox reaction represented by the following cell notation.

Fe(s) | Fe2+(aq) ‖ Cu2+(aq) | Cu(s)

 

a) Cu(s) + Fe2+(aq) → Fe(s) + Cu 2+(aq)

b) Fe(s) + Cu2+(aq) → Cu(s) + Fe 2+(aq)

c) 2 Fe(s) + Cu2+(aq) → Cu(s) + 2 Fe 2+(aq)

d) 2 Cu(s) + Fe2+(aq) → Fe(s) + 2 Cu 2+(aq)

e) 3 Fe(s) + 2 Cu2+(aq) → 2 Cu(s) + 3 Fe 2+(aq)