Electroplating turns electricity into a metal coating. Dial the current and time and see exactly how many grams of copper, silver, or gold plate out.
Electrolysis (Faraday's Laws)Live
electroplating by the numbers
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Faraday's laws tie electric charge to chemistry: the mass deposited equals (Q/F)·(M/z), where Q is total charge, F the Faraday constant, and z the ion charge. Double the current or time and you double the metal plated. Educational tool.
Reading this result: Passing 3600 C plates 1.185 g of Copper. Each Copper ion carries 2 electrons, so it takes 2× the charge to deposit one atom — a higher ion charge means less metal per coulomb, even at the same current.
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How it works
Faraday's laws connect charge to chemistry: the mass deposited equals (Q/F)·(M/z), where Q = current × time, F is the Faraday constant, M the molar mass, and z the ion charge. Doubling the current or the time doubles the metal plated — the quantitative basis of electroplating and refining. Educational tool.
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The solver uses established numerical methods, but results are for research and educational purposes and should be validated against experiment or professional review before you rely on them.