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: A spontaneous oxidation-reduction reaction involving zinc and copper.Why does the intensity of the blue solution color lessen as the reaction proceeds?

Problem

The figure shows a reaction between a zinc strip and Cu 2 plus ions in a solution. When the strip is immersed in the solution, zinc atoms on the surface of the strip transfer their electrons to the nearest Cu 2 plus ions (Zn is oxidized and Cu 2 plus is reduced) to produce Zn 2 plus ions and Cu atoms remaining attached to the strip. The overall reaction is: Zn left-parenthesis s right-parenthesis plus Cu 2 plus left-parenthesis aq right-parenthesis right arrow Zn 2 plus left-parenthesis aq right-parenthesis plus Cu left-parenthesis s right-parenthesis.

A spontaneous oxidation-reduction reaction involving zinc and copper.

Why does the intensity of the blue solution color lessen as the reaction proceeds?