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: Electrolytic cell with an active metal electrode. Nickel dissolves from the anode to form Ni2 + ( aq). At the cathode Ni2 + (aq) is reduced and forms a nickel "plate" on the steel cathode. Standard Re

Problem


A diagram shows a container filled with solution.  The nickel anode is attached to the positive end of the voltage source, and is where the following reaction takes place: Ni (solid) goes to Ni2+ (aqueous) plus 2 e-.  The steel object cathode is attached to the negative end of the voltage source, and is where the following reaction takes place: Ni2+ (aqueous) plus 2 e- goes to 2 Ni (solid).   Electrons travel from the anode to the cathode.
Electrolytic cell with an active metal electrode. Nickel dissolves from the anode to form Ni2 + ( aq). At the cathode Ni2 + (aq) is reduced and forms a nickel "plate" on the steel cathode.
 Standard Reduction Potentials in Water at 25°C 

Ered (V)Reduction Half-Reaction
-0.28Ni2+(aq)+2e- → (s)
+1.59NiO2(s)+4(aq)+2e- → 2+(aq)+2-(aq)
+0.442(s)+2(l)+2e- → 2(s)+2-(aq)


What E for this cell?