How many faradays of electricity are required to produce (a) 0.35 L of O₂ at exactly 1 atm and 25°C from aqueous H₂SO4 solution? faradays (b) 7.90 L of Cl₂ at 750 mm Hg and 20°C from molten NaCl? faradays (c) 4.8 g of Sn from molten SnCl₂? faradays A 215-mL solution of NaCl was electrolyzed for 6.10 min. If the pH of the final solution was 12.12, calculate the average current used. A

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.