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: Nickel and aluminum electrodes are used to build a galvanic cell. The standard reduction potential for the nickel(II) ion is -0.26 V and that of the aluminum(III) ion is -1.66 V.a. What is the theoret

Problem

Nickel and aluminum electrodes are used to build a galvanic cell. The standard reduction potential for the nickel(II) ion is -0.26 V and that of the aluminum(III) ion is -1.66 V.

a. What is the theoretical cell potential assuming standard conditions?

b. Which metal is the cathode?

c. Which statement is true?
     - Electrons flow from Ni to Al.
     - Electrons flow from Al to Ni.
     - The nickel electrode loses mass.
     - The aluminum electrode gains mass.

d. Type the shorthand notation for this cell. Do not include concentrations.

For example, in shorthand notation your answer might look like Cu|Cu | |Pd2+|Pd

Solution

(a) We’re being asked to determine the standard cell potential (E°cellof the reaction occurring in an electrochemical cell. To calculate for the standard cell potential, use the following equation:

https://lightcat-files.s3.amazonaws.com/problem_images/7e351f67feafeb34-1564509231807.jpg

Determine the anode and cathode by comparing their E° values.

 ↓ E° → oxidation → anode

 ↑ E° → reduction → cathode

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