1. What is Faraday's Second Law of Electrolysis?

Definition: Faraday's Second Law states that when the same quantity of electricity is passed through different electrolytes, the masses of substances deposited or dissolved at the electrodes are proportional to their equivalent weights.

Purpose: This calculator helps determine the mass of one ion (W₁) that would be deposited based on the mass of another ion (W₂) and their respective equivalent weights.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( W_1 \) — Mass of first ion (kg)
• \( E_1 \) — Equivalent weight of first substance (kg)
• \( E_2 \) — Equivalent weight of second substance (kg)
• \( W_2 \) — Mass of second ion (kg)

Explanation: The mass ratio of deposited substances equals the ratio of their equivalent weights when the same current is passed through them for the same time.

3. Importance of Faraday's Second Law

Details: This law is fundamental in electrochemistry, helping predict reaction outcomes, calculate required materials in electroplating, and determine unknown equivalent weights.

4. Using the Calculator

Tips: Enter the equivalent weights of both substances and the known mass of the second ion. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What is equivalent weight?
A: Equivalent weight is the molecular weight divided by the n-factor (number of electrons exchanged per molecule).

Q2: Can I use grams instead of kilograms?
A: Yes, as long as all inputs use the same unit, the result will be in that unit.

Q3: What's a typical equivalent weight?
A: For example, silver (Ag⁺) has 107.87 g/mol, copper (Cu²⁺) has 31.75 g/mol, and aluminum (Al³⁺) has 8.99 g/mol.

Q4: Does this apply to all electrolytes?
A: Yes, as long as the substances undergo complete electrolysis without side reactions.

Q5: How accurate is this calculation?
A: It's theoretically precise, but practical factors like current efficiency may affect real-world results.