Calculate the number of kilowatt-hours of electricity required to produce 1.0 x 103 kg of aluminum by electrolysis of Al* if the applied voltage is 4.50 V and the process is 45% efficient. (1 kWh = 3.6 x10° J and 1 J = 1C x 1V)

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2V0; (aq) +…

A: = 7.43 M[H+] = 1.74 M[VO2+] = 5.87 M[Fe2+] = 5.04 MT = 25oC=25+273=298Kn=2 as 2 electrons are…

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A: We wil calculate mass of Mg

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Q: An electrolysis cell for aluminum production operates at 5.5 V and a current of 7.0 x 10° A.…

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Q: An electrolysis cell for aluminum production operates at 5.0 V and a current of 3.0 × 10° A.…

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A:

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Q: A current of 4.71 A is passed through a Sn(NO3)2 solution. How long, in hours, would this current…

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A:

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Q: impure

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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.