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An aqueous solution is electrolysed so that exactly 0.5 mol of electrons are passed through the cell to bring about complete electrolysis. What is the total charge, in coulombs, required for this process? (Take Faraday constant F = 96500 C/mol.)

1. 24125
2. 48250
3. 96500
4. 193000

Correct answer: 48250

Solution

The quantity of electricity needed is fixed by the number of moles of electrons transferred. By Faraday's first law, Q = n(e-) * F. For 0.5 mol electrons, Q = 0.5 * 96500 = 48250 C.

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