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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

An Electrolytic Cell represents a non-spontaneous electrochemical cell

Examining an Electrolytic Cell

Concept #1: An Electrolytic Cell uses a non-spontaneous redox reaction in order to produce electricity.

Example #1: In a galvanic cell, the acceptance of an electron occurs at the ______ and in an electrolytic cell it occurs at the ______. 

a) cathode, cathode

b) anode, anode

c) anode, cathode

d) cathode, anode          

Concept #2: Although electrolytic cells have the same major components as galvanic cells, there are some key differences

Example #2: Which of the following is true about an electrolytic cell?

a) Has a positive cathode

b) Has no salt bridge

c) Cathode plates out

d) Has a negative anode 

Concept #3: An electrolytic cell uses non-spontaneous redox reactions.

Example #3: If the standard cell potential Eºcell for the given redox reaction is – 0.54 V, which of the following statements is true? z

Zn2+ (aq) + Ni (s) Zn (s) + Ni2+(aq)

a) The redox reaction will have an equilibrium constant value that is greater than 1. 

b) The redox reaction will produce electricity. 

c) The redox reaction will have an equilibrium constant value that is less than 1.

d) The reaction quotient will be less than the equilibrium constant. 

If the overall redox reaction for an electrolytic cell is given below, what will happen to the mass of the cobalt electrode?

Co2+ (aq) + Cu (s) ⇌ Co (s) + Cu2+(aq)