A Coulomb is a measurement of electric charge in the SI (Système international d'unités -- International System of Units). The Coulomb usually is first encountered in introductory chemistry or electronics courses, as it directly relates amperes to the charge of elementary particles. The Faraday is a unit of charge reflecting the strength of charge in one mole of a substance. These units often are converted between each other to determine various characteristics about a given chemical reaction or its accompanying electrical discharge.
Instructions
-
-
1
Divide the number of Coulombs by the number of moles of elementary charge associated with the reaction. The moles of elementary charge can be determined experimentally or retrieved from chemical reference sources.
-
2
Multiply the resulting value by the conversion factor of Coulombs to Faradays -- 1 Coulomb equals 96485.33 Faradays.
-
-
3
Simplify the resulting fraction, if necessary, to determine the number of Coulombs in a Faraday for the elementary particles in question.