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 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?

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 cell operat

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?

Solution

We’re being asked to determine which electrode loses mass as the reaction proceeds. We’re given the following diagram:

Recall that a voltaic or galvanic cell is an electrochemical cell that is spontaneous and produces electricity


Let's recall some parts of the galvanic cell:

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