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: The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one half-reaction isMn2+(aq) + 2H2O(l) ⟶ MnO2(s) + 4H+(aq) + 2e−If a current of 25.0 A is used, how many hour

Problem

The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one half-reaction is

Mn2+(aq) + 2H2O(l) ⟶ MnO2(s) + 4H+(aq) + 2e

If a current of 25.0 A is used, how many hours are needed to produce 1.00 kg of MnO  2? At which electrode is the MnO2 formed?