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Faraday's Electrolysis Law:
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Faraday's law of electrolysis states that the amount of substance produced at an electrode during electrolysis is directly proportional to the quantity of electricity that passes through the electrolyte. The fundamental equation is Q = n × F, where Q is the electric charge, n is the number of moles of electrons, and F is Faraday's constant.
The calculator uses Faraday's electrolysis equation:
Where:
Explanation: This equation calculates the total electric charge required to electrolyze a given number of moles of substance, based on Faraday's constant which represents the charge of one mole of electrons.
Details: Accurate charge calculation is essential for determining the amount of material deposited or dissolved during electrolysis processes, which is crucial in electroplating, electrorefining, and electrochemical manufacturing processes.
Tips: Enter the number of moles and Faraday's constant (default value is 96485 C/mol). Both values must be positive numbers.
Q1: What is the exact value of Faraday's constant?
A: Faraday's constant is approximately 96485.33212 C/mol, which is the electric charge of one mole of electrons.
Q2: Can this calculator be used for different substances?
A: Yes, the equation Q = n × F applies to all electrolysis processes, as it calculates the fundamental charge required regardless of the specific substance.
Q3: How is this related to the mass of substance deposited?
A: The mass deposited can be calculated using m = (Q × M) / (z × F), where M is molar mass and z is the number of electrons transferred per ion.
Q4: What are typical applications of this calculation?
A: This calculation is used in electroplating, battery technology, corrosion studies, and industrial electrochemical processes.
Q5: Are there any limitations to this equation?
A: The equation assumes 100% current efficiency. In practical applications, side reactions and inefficiencies may require adjustments to the calculated values.