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: Concentration cell based on the Ni2+-Ni cell reaction. (a) Concentrations of Ni2+(aq) in the two half-cells are unequal, and the cell generates an electrical current and a voltage. (b) The c

Problem

Two diagrams show two beakers, connected by a salt bridge and a wire.  The beaker on the left contains an Ni anode and the beaker on the right contains an Ni cathode. a) The left (anode) beaker contains a 1.00 times 10-3 molar Ni2+ concentration, and the right (cathode) beaker contains a 1.00 molar Ni2+ concentration. Electrons travel left to right through a wire from the Ni anode to the Ni cathode, producing 0.09 volts. b) After discharge, the Ni2+ concentration in both beakers is 0.5 molar and no voltage is produced.

Concentration cell based on the Ni2+-Ni cell reaction. (a) Concentrations of Ni2+(aq) in the two half-cells are unequal, and the cell generates an electrical current and a voltage. (b) The cell operates until [Ni2+] is the same in the two half-cells, at which point the cell has reached equilibrium and the emf goes to zero.

Which electrode, if any, loses mass as the reaction proceeds?