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: Consider a fuel cell that uses the reaction of ethanol with oxygen to produce electricity, CH3CH2OH(l) + 3O2(g) → 2CO2(g)+ 3H2O(l)Determine the E°cell for this cell at 25°.E°cell = v

Solution: Consider a fuel cell that uses the reaction of ethanol with oxygen to produce electricity, CH3CH2OH(l) + 3O2(g) → 2CO2(g)+ 3H2O(l)Determine the E°cell for this cell at 25°.E°cell = v

Problem

Consider a fuel cell that uses the reaction of ethanol with oxygen to produce electricity, 

CH3CH2OH(l) + 3O2(g) → 2CO2(g)+ 3H2O(l)

Determine the E°cell for this cell at 25°.

cell = v

Solution

We’re asked to calculate the cell potential (E°cell)­ of a fuel cell. The cell potential of an electrochemical cell is related to Gibb's free energy of the reaction by the following equation:

∆G° = Gibb’s Free Energy
n = number of electrons transferred
= Faraday’s constant = 96485 C/(mol e-)
cell =standard cell potential

We will solve the problem in the following steps:

1. Calculate ΔG˚rxn (since it is not given)
 2. Determine the number of electrons involved in the reaction by balancing the redox reaction
 3. Calculate E˚cell using the equation above.

View the complete written solution...