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 the voltaic cell illustrated in the figure , which is based on the cell reaction Zn(s) + Cu2 +  (aq)  →  Zn2 +  (aq) + Cu(s).Under standard conditions, what is the maximum electrical work, in joules, that the cell can accomplish if 50.0 g of copper is plated out?

Solution: Consider the voltaic cell illustrated in the figure , which is based on the cell reactionZn(s) + Cu2 +  (aq)  →  Zn2 +  (aq) + Cu(s).Under standard conditions, what is the maximum electrical work, in

Problem

Consider the voltaic cell illustrated in the figure The figure shows a voltaic cell where Zn is the anode and Cu is the cathode. A voltmeter depicts the value equal to 1.10. Solid Zn loses two electrons to form an aqueous Zn two plus ion. An aqueous Cu two plus ion gains two electrons to form solid Cu., which is based on the cell reaction
Zn(s) + Cu2 +  (aq)  →  Zn2 +  (aq) + Cu(s).

Under standard conditions, what is the maximum electrical work, in joules, that the cell can accomplish if 50.0 g of copper is plated out?