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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

Electroplating involves coating an electrode through the use of current

Electrochemical Stoichiometry

Concept #1: Electrical current (A) is the rate at which electrons move from electrode to electrode.

Example #1: Determine the electrical current produced if a charge 4.14 x 103 C passes through a wire for 15 mins.

Concept #2: Electrochemical Stoichiometry deals with calculations in electrochemical cells that involve current and charge.

Example #2: Gold can be plated out of a solution containing Au3+ based on the following half reaction: 

Au3+ (aq) + 3 e  →. Au (s)

What mass of gold is plated by a 41 minute flow of 6.8 A current?

Concept #3: When the initial mass for a half reaction is given we can utilize the mass version of the stoichiometric chart to find time.

Example #3: How much time (in hours) would it take to plate out 42.1 g nickel using a current of 3.08 A?

Ni2+ (aq) + 2 e  →. Ni (s)

Practice: Cu2+ is reduced to Cu(s) at an electrode. If a current of 1.25 A is passed for 72 hours, what mass of copper is deposited at the electrode? (MW of Cu: 63.55 g/mol)

Practice: A solution of Mn+5 is used to plate out Mn in an electrochemical cell. If a total of 1.13 g of Mn is plated out in a total time of 1600 seconds, what was the electrical current used? (MW of Mn is 54.94 g/mol)