Electrochemistry

Electrochemistry : the study of the interchange of chemical and electrical energy
Redox reaction : a transfer of electrons from the reducing agent to the oxidizing agent
Oxidation: a loss of electrons (an increase in the oxidation number)
Reduction: a gain of electrons (a decrease in the oxidation number)
Half-reactions: a redox reaction broken in to two parts, one half with the oxidation and the other half with the reduction
Salt bridge: the connection between the two solutions
Galvanic cell: device in which chemical energy is changed to electrical energy
Anode: the electrode at which oxidation occurs (an-ox)
Cathode: the electrode at which reduction occurs (red-cat)
Cell potential, (Ecell): potential difference between the oxidation and reduction
Volt: the unit of electrical potential (J/C)
Standard hydrogen electrode: a platinum electrodes in contact with 1M H+ ions bathed by H2 gas at 1 atm
Standard reduction potentials, E : likelihood for the reduction to occur with all solutes at 1M or 1 atm
Concentration cell: cell with both electrodes having identical components but at different concentrations
Nernst equation: converts cells that are at nonstandard conditions to standard conditions E = E - ln(Q) RT nF
Glass electrode: contains a reference solution of dilute hydrochloric acid in contact with a thin glass membrane
Lead storage battery: lead serves as the anode and lead coated with lead dioxide serves as the cathode
Electrolytic cell: an apparatus that uses electrical energy to produce chemical change for nonspontaneous cells
Electrolysis: forcing a current through a cell to produce a chemical change ; used for nonpontaneous cells
Ampere: measure of current in coulombs per second (C/s). Often used to help convert the number of electrons flowing (current) to the rate of reaction in time
Electrochemistry:
Introduction
Chemical reactions which have the capacity to occur spontaneously are in a position to generate electrical energy under appropriate conditions. Chemical reactions or processes which do not have the capacity to take place spontaneously can be induced to do so if an appropriate quantity of electrical energy is supplied under appropriate conditions. Both types of chemical changes are regarded as being Electrochemistry : the study of the interchange of chemical and electrical energy
Redox reaction : a transfer of electrons from the reducing agent to the oxidizing agent
Oxidation: a loss of electrons (an increase in the oxidation number)
Reduction: a gain of electrons (a decrease in the oxidation number)
Half-reactions: a redox reaction broken in to two parts, one half with the oxidation and the other half with the reduction
Salt bridge: the connection between the two solutions
Galvanic cell: device in which chemical energy is changed to electrical energy
Anode: the electrode at which oxidation occurs (an-ox)
Cathode: the electrode at which reduction occurs (red-cat)
Cell potential, (Ecell): potential difference between the oxidation and reduction
Volt: the unit of electrical potential (J/C)
Standard hydrogen electrode: a platinum electrodes in contact with 1M H+ ions bathed by H2 gas at 1 atm
Standard reduction potentials, E : likelihood for the reduction to occur with all solutes at 1M or 1 atm
Concentration cell: cell with both electrodes having identical components but at different concentrations
Nernst equation: converts cells that are at nonstandard conditions to standard conditions E = E - ln(Q) RT nF
Glass electrode: contains a reference solution of dilute hydrochloric acid in contact with a thin glass membrane
Lead storage battery: lead serves as the anode and lead coated with lead dioxide serves as the cathode
Electrolytic cell: an apparatus that uses electrical energy to produce chemical change for nonspontaneous cells
Electrolysis: forcing a current through a cell to produce a chemical change ; used for nonpontaneous cells
Ampere: measure of current in coulombs per second (C/s). Often used to help convert the number of electrons flowing (current) to the rate of reaction in time
Electrochemistry:
Introduction
Chemical reactions which have the capacity to occur spontaneously are in a position to generate electrical energy under appropriate conditions. Chemical reactions or processes which do not have the capacity to take place spontaneously can be induced to do so if an appropriate quantity of electrical energy is supplied under appropriate conditions. Both types of chemical changes are regarded as being