Electrolysis and Faraday's Law
In electrolysis, the amount of substance produced is set by the charge passed, via Faraday's law. The ladder runs: charge = current × time (in seconds); moles of electrons = charge ÷ F (Faraday's constant); moles of metal = moles of electrons ÷ (electrons per ion); and finally grams = moles × molar mass.
The traps drop or swap units along the ladder — taking moles of electrons as moles of metal (divide by the electron count per ion), using charge as moles (divide by F), plugging minutes in as seconds, or reporting moles where grams were asked (convert with molar mass). Carry each step through to the requested unit.
The work
3 ways in · any order
Lesson
Electrolysis & Faraday's Law
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Faraday's law converts charge (current × time) to moles of electrons, then to moles of metal, then grams. The lesson climbs the ladder with correct units, then closes with a ten-scenario check.
Diagnostic
10-item topic check
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Ten items spanning the Topic 9.11 misconceptions: Faraday-ladder unit and step errors (electrons vs metal, charge vs moles, minutes vs seconds), and the final quantity reported in the wrong units.
Targeted Practice
Drill a single misconception
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Pick one of the failure modes you missed and drill it on its own. The round is adaptive: two correct in a row clears the misconception and moves you to the next.