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: Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution:c. CuBr2(aq)

Problem

Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution:

c. CuBr2(aq)

Solution

We’re being asked to determine the cathode and anode half-reactions for the electrolysis of an aqueous CuBr2 solution


Recall that the cathode is where reduction occurs while the anode is where oxidation occurs.


Since CuBr2 is an ionic compound, it forms ions when dissociating in water

The dissociation of CuBr2 in water is as follows:

The bromide ion, Br, has a charge of –1. Copper then has a charge of +2:

CuBr2(s)  Cu2+(aq) + 2 Br(aq)


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