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: A Cu-Zn voltaic cell based on the reaction in the equation given below. Zn( s ) + Cu2 +  ( aq )  →  Zn2 +  ( aq ) + Cu( s )Which metal is oxidized in this voltaic cell?

Solution: A Cu-Zn voltaic cell based on the reaction in the equation given below.Zn( s ) + Cu2 +  ( aq )  →  Zn2 +  ( aq ) + Cu( s )Which metal is oxidized in this voltaic cell?

Problem

A photograph shows a voltmeter attached to a Zn electrode in a 1 molar ZnSO4 solution, and a Cu electrode in a 1 molar CuSO4 solution. The two solutions are in contact with each other through a porous glass disc.
A Cu-Zn voltaic cell based on the reaction in the equation given below.
Zn( s ) + Cu2 +  ( aq )  →  Zn2 +  ( aq ) + Cu( s )

Which metal is oxidized in this voltaic cell?

Solution

We’re being asked to determine which metal is being oxidized given the following reaction.

Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)


Recall the mnemonics LEO GER.

Lose               Gain

Electron         Electrons

Oxidation       Reduction


We’ll identify the anode and cathode half-reactions using the following steps.

Step 1. Separate the overall reaction into two half-reactions
Step 2. Balance the elements in each half-reaction.

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