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 cell notation for the redox reaction given below      3 Cl2(g) + 2 Fe(s) → 6 Cl − (aq) + 2 Fe3+(aq) A) Fe(s) | Fe3+(aq) || Cl2(g), Cl −(aq) | Pt B) Cl − (aq) | Cl2(g) | Pt || Fe3+(aq)

Problem

Determine the cell notation for the redox reaction given below

     3 Cl2(g) + 2 Fe(s) → 6 Cl  (aq) + 2 Fe3+(aq)

A) Fe(s) | Fe3+(aq) || Cl2(g), Cl (aq) | Pt

B) Cl  (aq) | Cl2(g) | Pt || Fe3+(aq) | Fe(s)  

C) Fe(s) | Fe3+(aq) || Cl2(g) | Cl  (aq) | Pt

D) Fe(s) | Cl2(g) || Fe3+(aq) | Cl  (aq) | Pt

E) Pt | Cl2(g) | Cl  (aq) || Fe3+(aq) | Fe(s)