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The first of these laws relates the products formed by electrolysis to the amount of electricity run through the initial substance. The equation is as follows:
The first of these laws relates the products formed by electrolysis to the amount of electricity run through the initial substance. The equation is as follows:
m = ZIt
m = ZIt
where m is the mass of the product in grams, I is the current of electricity in amperes, t is the time in seconds it took to produce the end result of the reaction, and Z is the constant of proportionality. The constant of proportionality is also called the electrochemical equivalent <ref>Ahmad, Zaki. Principles of Corrosion Engineering and Corrosion Control. Butterworth-Heinemann, 2006.</ref>. The electrochemical equivalent varies from metal to metal. According to Faraday’s first law of electrolysis, the mass of primary product is directly proportional to the amount of electricity used during electrolysis.
where m is the mass of the product in grams, I is the current of electricity in amperes, t is the time in seconds it took to produce the end result of the reaction, and Z is the constant of proportionality. The constant of proportionality is also called the electrochemical equivalent. The electrochemical equivalent varies from metal to metal. According to Faraday’s first law of electrolysis, the mass of primary product is directly proportional to the amount of electricity used during electrolysis.
Faraday’s second law of electrolysis relates the mass of the product of electrolysis to molar mass, the number of electrons, and the electrochemical equivalent, stating that the mass of the primary product in grams is directly proportional to the electrochemical equivalent as well as the ratio of molar mass to number of electrons in a reaction.
Faraday’s second law of electrolysis relates the mass of the product of electrolysis to molar mass, the number of electrons, and the electrochemical equivalent, stating that the mass of the primary product in grams is directly proportional to the electrochemical equivalent as well as the ratio of molar mass to number of electrons in a reaction.