Faraday's Second Law Formula:
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Definition: Faraday's Second Law states that when the same quantity of electricity is passed through different electrolytes, the masses of ions deposited or liberated are proportional to their equivalent weights.
Purpose: This calculator helps determine the mass of a second ion produced or consumed in electrolysis based on the mass of a first ion and their equivalent weights.
The calculator uses the formula:
Where:
Explanation: The mass of the second ion is calculated by multiplying the mass of the first ion by the ratio of their equivalent weights.
Details: This law is fundamental in electrochemistry for determining quantities of substances produced or consumed in electrolytic processes, with applications in electroplating, battery technology, and industrial electrolysis.
Tips: Enter the mass of the first ion (W₁), equivalent weight of substance 1 (E₁), and equivalent weight of substance 2 (E₂). All values must be > 0. Default values are provided for common substances.
Q1: What is equivalent weight?
A: Equivalent weight is the molecular weight divided by the number of electrons transferred per molecule in the reaction (valency).
Q2: Can I use grams instead of kilograms?
A: Yes, as long as all weights are in the same units, the calculator will work correctly.
Q3: What are typical equivalent weights?
A: For example, silver (Ag⁺) has 0.1079 kg, copper (Cu²⁺) has 0.0318 kg, and zinc (Zn²⁺) has 0.0327 kg.
Q4: Does this work for gases produced in electrolysis?
A: Yes, the law applies to both solid deposits and gases liberated during electrolysis.
Q5: How accurate is this calculation?
A: The calculation is theoretically exact, but practical results may vary slightly due to side reactions or inefficiencies.