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ChemistryNEET 2024Electrolysis and Faraday's laws; batteries and corrosion

Electrochemistry

The mass in grams of copper deposited by passing a current of 9.6487 A through a voltameter containing copper sulphate solution for 100 seconds is (given molar mass of Cu = 63 g mol−163\ \mathrm{g\,mol^{-1}}, 1 F = 96487 C):

  1. A.0.315 g✓
  2. B.31.5 g
  3. C.0.0315 g
  4. D.3.15 g

Solution

Charge =It=9.6487×100=964.87= It = 9.6487 \times 100 = 964.87 C =0.01= 0.01 F. Copper needs 2 F per mole, so 0.0050.005 mol is deposited: 0.005×63=0.3150.005 \times 63 = 0.315 g.

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