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A Level Chemistry | Electrochemistry 9 | Electrolysis | Faraday Constant

Welcome to A Level Electrochemistry (Part 9)! In this session, we continue with Electrolysis and introduce the important concept of the Faraday Constant, which helps calculate the amount of substance produced during electrolysis — a key numerical topic in A Level exams.

1️⃣ Recap: What is Electrolysis? –
Electrolysis is the use of electrical energy to drive a non-spontaneous redox reaction. Oxidation occurs at the anode and reduction at the cathode.

2️⃣ Introduction to the Faraday Constant (F) –
The Faraday constant represents the charge carried by one mole of electrons. Its value is 96,500 C mol⁻¹ and it links electrical charge to chemical change.

3️⃣ Relationship Between Charge, Current & Time –
Students learn the key formula:
Q = I × t
Where Q = charge (Coulombs), I = current (Amperes), and t = time (seconds).

4️⃣ Using Faraday’s Law in Calculations –
We explain how to calculate the amount of substance formed using:
moles of electrons = Q / F
and link this to stoichiometry of half-equations.

5️⃣ Predicting Mass or Volume Formed –
Students practise calculating the mass of metal deposited or gas produced during electrolysis — a common exam numerical.

6️⃣ Past Paper Techniques & Common Mistakes –
Common errors include incorrect unit conversion, forgetting electron ratios, and not using the correct number of moles of electrons in half-equations.

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