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: Given that E°cell = 3.20V for the reaction 2Na(in Hg) + Cl2(g) ⇌ 2Na+(aq) + 2Cl−(aq)What is E° for the reduction 2Na+(aq) + 2e−→ 2Na(in Hg)?


Given that E°cell = 3.20V for the reaction 2Na(in Hg) + Cl2(g) ⇌ 2Na+(aq) + 2Cl(aq)

What is E° for the reduction 2Na+(aq) + 2e→ 2Na(in Hg)?


We’re being asked to determine the standard reduction potential (E°red) of Na+/Na (inHg) from a reaction occurring in an electrochemical cell. To calculate for the standard reduction potential, use the following equation:

When a balanced reaction is given, identify the anode and the cathode half-reactions by determining the changes in oxidation states of each species based on the given reaction:


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