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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
Standard Reduction Potentials
Intro to Electrochemical Cells
Galvanic Cell
Electrolytic Cell
Cell Potential: Standard
Cell Potential: The Nernst Equation
Cell Potential and Gibbs Free Energy
Cell Potential and Equilibrium
Cell Potential: G and K
Cell Notation

Standard Reduction Potentials measure how easily a species can accept electron(s) from another species

Understanding Standard Reduction Potentials

Concept #1: The Standard Reduction Potential (Eºred) is measured under standard conditions: 25ºC, 1 atm, 1 M solution and pH = 7.

Recall, oxidation involves losing electrons and reduction involves gaining electrons.

Concept #2: The greater the Eºred the more likely reduction will occur.

Example #1: Determine which of the following will least likely donate an electron?

a) H2                         b) Br2                        c) Zn2+                      d) Cl2                        e) Li+ 

Rank the given metal ions in order of increasing strength as an oxidizing agent.

Pb2+ (-0.13 V), Mn2+ (-1.18 V), Cu2+ (+0.16 V), Co3+ (+1.82 V), Fe3+ (+0.77 V)

Determine which species can oxidize Br2.