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To determine the value of Faraday constant (quantity of electricity per mole) by using electrolysis of Copper.
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1) Title: QN1 A Quantitative study of electrolysis 2) Aim/Objective: To determine the value of Faraday constant (quantity of electricity per mole) by using electrolysis of Copper. 3) Results: Before electrolysis: Weight of cathode = 2.164 g Weight of anode = 2.502 g After electrolysis: Weight of cathode = 2.237 g Weight of anode = 2.435 g Time of electrolysis = 20 minutes = 1200 seconds Ammeter reading = 0.19A 4) Calculation/interpretation: The equation of the electrolysis reaction at the cathode: Cu2+(aq.) + 2e- › Cu(s.) Gain in weight of cathode = 2.237g - 2.164g = 0.073 g Loss in weight of anode = 2.520 - 2.435g = 0.085 g No. of moles of loss in cupper anode = 0.085 / 63.5 = 0.00134 mol Quantity of electricity required = 0.00134 mol * 2 = 0.00268 mol Quantity of electricity supplied = 1200 * 0.19 = 228C Faraday Constant = quantity of electricity / no. of moles =...
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