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118 Terms
Electrochemistry
The branch of chemistry that deals with the relationship between electricity and chemical reactions.
Electrochemical Cells
Devices that convert chemical energy into electrical energy or vice versa.
Galvanic Cell (Voltaic Cell)
A type of electrochemical cell that uses a spontaneous reaction to generate electrical energy.
Electrolytic Cell
A type of electrochemical cell that uses electrical energy to drive a nonspontaneous reaction.
Anode
The electrode where oxidation occurs in an electrochemical cell.
Cathode
The electrode where reduction occurs in an electrochemical cell.
Half-Reaction
The individual oxidation or reduction reaction that occurs at an electrode in an electrochemical cell.
Salt Bridge
A component in an electrochemical cell that allows ions to flow between the two half-cells, maintaining charge balance.
Cell Diagram
A notation that describes the components and arrangement of an electrochemical cell.
Cell Potential
The voltage across the electrodes of a galvanic cell, also known as cell voltage or electromotive force (emf).
Standard Cell Potential
The cell potential under standard conditions, including a temperature of 25˚ Celsius, 1 M concentration of reactants and products, and 1 atm pressure.
Standard Reduction Potential
The voltage associated with a reduction reaction at an electrode under standard-state conditions.
Standard Hydrogen Electrode (SHE)
The reference electrode used to measure standard reduction potentials, with a defined potential of zero.
Standard-State Values
The values of electrode potentials for half-reactions under standard conditions.
Half-Reaction
A chemical reaction that involves the transfer of electrons.
E°(V)
The standard electrode potential, measured in volts (V).
Cu2+(aq)
Copper ion in aqueous solution.
Cu+(aq)
Copper ion in aqueous solution with a +1 charge.
Sn4+(aq)
Tin ion in aqueous solution with a +4 charge.
Sn2+(aq)
Tin ion in aqueous solution with a +2 charge.
F2(g)
Fluorine gas.
F(aq)
Fluoride ion in aqueous solution.
O3(g)
Ozone gas.
O2(g)
Oxygen gas.
H2O
Water.
H2(g)
Hydrogen gas.
Pb(s)
Solid lead.
H2O2(aq)
Hydrogen peroxide in aqueous solution.
Sn(s)
Solid tin.
PbO(s)
Lead(II) oxide.
PbSO4(s)
Lead(II) sulfate.
Ni(s)
Solid nickel.
Ce++(aq)
Cerium ion in aqueous solution with a +2 charge.
Co2+(aq)
Cobalt ion in aqueous solution with a +2 charge.
Mn2+(aq)
Manganese ion in aqueous solution with a +2 charge.
Fe(s)
Solid iron.
Cr*(aq)
Chromium ion in aqueous solution with a +3 charge.
Br2(1)
Bromine gas.
NO(g)
Nitric oxide gas.
Ag*(aq)
Silver ion in aqueous solution.
Na*(aq)
Sodium ion in aqueous solution.
Fe3+(aq)
Iron ion in aqueous solution with a +3 charge.
Ca2+(aq)
Calcium ion in aqueous solution with a +2 charge.
Sr2+(aq)
Strontium ion in aqueous solution with a +2 charge.
MnO4(aq)
Permanganate ion in aqueous solution.
Ba2+(aq)
Barium ion in aqueous solution with a +2 charge.
I2(s)
Iodine solid.
K+(aq)
Potassium ion in aqueous solution.
Li*(aq)
Lithium ion in aqueous solution.
AgCl(s)
Silver chloride solid.
Ecell
The measured electromotive force, or cell potential, of a galvanic cell.
Spontaneity
The tendency of a reaction to occur without external influence.
E° values
The standard electrode potentials for half-cell reactions.
Anode
The electrode where oxidation occurs in a galvanic cell.
Cathode
The electrode where reduction occurs in a galvanic cell.
Stoichiometric coefficients
The numbers that appear in front of chemical formulas in a balanced equation.
Intensive properties
Properties that do not depend on the size or amount of a substance.
ΔG
The change in Gibbs free energy of a reaction.
ΔS
The change in entropy of a reaction.
Emf
The electromotive force, or cell potential, of a galvanic cell.
System
The chemical reaction or process being studied.
Surroundings
Everything outside of the system in a chemical reaction or process.
Free energy
The energy available to do work in a chemical reaction or process.
Spontaneous reaction
A reaction that occurs without external influence.
Ecell
The cell potential of a galvanic cell.
ΔG
The change in Gibbs free energy of a reaction.
Gibbs free energy
A thermodynamic potential that measures the maximum amount of useful work that can be obtained from a system.
Reaction
A process in which one or more substances are converted into different substances.
Ecell
The cell potential of a galvanic cell.
ΔG
The change in Gibbs free energy of a reaction.
Spontaneous
A reaction that occurs without external influence.
AG
The change in Gibbs free energy of a reaction.
n
The number of moles of electrons in a reaction.
F
Faraday constant, equal to 96,500 C/mol.
RT
The product of the gas constant (R) and temperature (T).
In K
The natural logarithm of the equilibrium constant (K).
AG°
The standard change in Gibbs free energy of a reaction.
In K
The natural logarithm of the equilibrium constant (K).
K
The equilibrium constant of a reaction.
n
The number of moles of electrons in a reaction.
AG°
The standard change in Gibbs free energy of a reaction.
RT
The product of the gas constant (R) and temperature (T).
In K
The natural logarithm of the equilibrium constant (K).
AG°
The standard change in Gibbs free energy of a reaction.
Ecell
The cell potential of a galvanic cell.
Standard-State Conditions
The conditions under which standard electrode potentials are measured.
Negative
Indicates that the electrical work is done by the system on the surroundings.
Free energy
The energy available to do work in a chemical reaction or process.
ΔG
The change in Gibbs free energy of a reaction.
Ecell
The cell potential of a galvanic cell.
ΔG
The change in Gibbs free energy of a reaction.
Ecell
The cell potential of a galvanic cell.
K
The equilibrium constant of a reaction.
Direction of Reaction
The direction in which a reaction will proceed based on the values of AG and E°cell.
K
The equilibrium constant of a reaction.
E°cell
The standard cell potential of a galvanic cell.
RT
The product of the gas constant (R) and temperature (T).
F
Faraday constant, equal to 96,500 C/mol.
Ecell
The cell potential of a galvanic cell.
Standard-State Conditions
The conditions under which standard electrode potentials are measured.
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