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Moles of electrons One Faraday is the amount of electricity that corresponds to one mole of electrons flowing around an electrical circuit (such as an electrolysis cell) In electrolysis we use half-equations to show what happens at each electrode. For example in electrolysis of brine: ANODE: 2Cl-Cl2+2e- “Two moles of chloride ions are oxidised to form one mole of chlorine molecules, and two Faradays of electrons flows from the anode around the circuit to the power supply” CATHODE: 2H+ + 2e- H2 “Two Faradays of electrons flows into the cathode from the power supply, allowing two moles of hydrogen ions to be reduced to form one mole of hydrogen molecules” Calculations involving Faradays e.g. 0.5 Faradays of electrons flow into the cathode during electrolysis of a copper sulphate solution. What mass of copper could be deposited on the cathode? At the cathode: Cu2+ + 2e- Cu Ratio 1:2:1 Moles of electrons = 0.5 (1 Faraday = 1 mole of electrons) Mole ratio = 2 : 1 electrons : Cu So moles of Cu = 0.25 MassofCu=molesofCuxAr ofCu = 0.25x64 = 16gPDF Image | Electrolysis is using an electric current
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