Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 15 minutes at a current of 3.2 A given the following reaction. Z3+(aq) + 3e- → Z(s) Atomic Mass: Z: 205.44 g/mol Round your answer to 2 decimal places.

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 17…

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Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 17…

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A: 3.4 amperes is 3.4 coulombs per second, 5C/s So the total charge in 20 minutes is Q = 3.4C/s x 20min…

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Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 15…

A: Given :  Current (I) = 2.6 A  Time(t) = 15 min = 900 sec  Atomic mass of Z = 182.54 g/mol

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Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 15…

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Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 17…

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Q: Enter your answer in the provided box. Copper is purified by electrolysis. A 4.75-kg anode is used…

A: Given:  Mass of anode = 4.75 kg = 4750 gm  Current (I) = 37.8 A

Q: mass

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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.