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: What is the balanced half‐reaction that occurs at the anode in the unbalanced overall cell reaction of a voltaic cell: 3 MnO4– + 5 Fe (s) → 3 Mn2+ + 5 Fe3+ a) MnO 4- (aq) + 8H (aq) + 5e - → Mn2+ (aq

Problem

What is the balanced half‐reaction that occurs at the anode in the unbalanced overall cell reaction of a voltaic cell:

3 MnO4+ 5 Fe (s) → 3 Mn2+ + 5 Fe3+

a) MnO 4- (aq) + 8H (aq) + 5e - → Mn2+ (aq) + 4H 2 O(l) 

b) 2MnO 4- (aq) +12H+ (aq) + 6e - → 2Mn2+ (aq) + 3H 2 O(l)

c) Fe(s) → Fe3+ (aq) + 3e -

d) Fe(s) → Fe2+ (aq) + 2e -

e) Fe2+ (s) → Fe3+ (aq) + e -