Faraday's Laws of Electrolysis
Use Faraday's laws to calculate the amount of substance deposited or liberated during electrolysis and understand the quantitative aspects of electrolysis.
Why this shows up in the exam
NEET/JEE regularly test your ability to solve numerical problems based on Faraday's laws and electrolysis stoichiometry.
How NEET tests this
Practise it
These are real questions from past NEET papers that test this exact idea.
During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is
Push further
More challenging4 harder questions built from the past papers above — a step up in difficulty, with distractors designed so you can't get there by elimination. Written and checked by our reviewers, not from a real paper.
How many Faradays of electricity are required to deposit 27 g of aluminium from molten AlCl₃? (Atomic mass of Al = 27 g mol⁻¹)
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