Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous solution containing M2X1 (where X is the anion) with a supplied current of 6.2 A for 11 h, consuming 0.2406 kWh of electrical energy. Assume that the current efficiency is 96%.

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 = 7.33 A Time passed = 10 hour Power = 0.2229 KWh. Current efficiency = 81 %

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

A:

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

A: Electrical energy=0.1599 kWh

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

A: Given: Current = 5.72 A Time passed = 8 hour Power = 0.2293 KWh. Current efficiency = 91 %

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

A: Answer: Given current efficiency is 96%, therefore actual current passed…

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…

A: Answer: Since, given current efficiency is 87%, therefore actual current passed through the solution…

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

A: Electrical energy=0.2411 kWh

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

A: Electrical energy=0.2287 kWh

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

A: Given: Current = 5.72 A Time passed = 8 hour Power = 0.2293 KWh. Current efficiency = 91 %

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

A: Given: Current = 5.56 A Time passed = 10 hour Power = 0.2196 KWh. Current efficiency = 94 %

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

A:

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

A: Let voltage required is V volt . And we are given 91%effeicient current = 6.82 ,so nett effective…

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

A:

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: 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…

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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.