Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous solution containing M2X2 (where X is the anion) with a supplied current of 5.92 A for 12 h, consuming 0.1731 kWh of electrical energy. Assume that the current efficiency is 87%. (Input values only with 2 decimal places).

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Q: ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited…

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Q: ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited…

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Q: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous…

A: Given: Current = 5.92 A Time passed = 12 hour Power = 0.1731 KWh. Current efficiency = 87 %

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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.