Chapter 9: Production of chemicals by electrolysis Flashcards
Electrolysis
A process which produces a non-spontaneous redox reaction by the passage of electrical energy from a power supply through a conducting liquid.
Electrolytic cell
A cell in which electrolysis can occur.
Electrolyte
A chemical substance that conducts electric current as a result of dissociation into positively and negatively charged ions, which migrate towards the negative and positive terminals of an electric circuit.
Cathode
An electrode at which a reduction reaction occurs.
Anode
An electrode at which an oxidation reaction occurs.
Non-spontaneous Reaction
A reaction which would not normally occur without the application of electrical energy. It is the reverse of a spontaneous reaction which produces electrical energy.
Spontaneous Reaction
A reaction which occurs naturally, either in electrochemical cells or when chemicals are mixed directly. The reaction does not need to be driven by an external source of power.
Reactive electrode
An electrode which is consumed in an electrochemical cell reaction.
Electro-chemical cell
A device that converts chemical energy into electrical energy, or vice versa.
Brine
A concentrated sodium chloride solution.
Semi-permeable Membrane
A membrane that will only allow certain molecules or ions to pass through it.
Electroplating
Also known as deposition, a process which uses electrolysis to deposit a layer of metal on the surface of another material.
Coulomb
A unit of charge, symbol C. It is the quantity of charge conveyed in one second by one ampere of current.
Faraday’s First Law of Electrolysis
The mass of metal produced at the cathode is directly proportional to the electrical charge passed through the cell. It may be written as m is proportional to Q.
Faraday
The charge on one mole of electrons, symbol F. One faraday has a charge of 96500 Coulombs.
