A current of 0.452 Amps is passed through an electrolytic cell containing molten CaCl2 for 1.50 hrs. Write the electrode reactions (at both the Anode and the cathode electrodes) and calculate the quantity of products (in grams) formed at each electrodes.

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Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

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Q: your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Given,produced volume of Cl2 gas at anode ( at STP ) = 4.18 Ltime taken = 16 h.

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Q: Define what is meant by standard cell.

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A: Given, Current passing = 330 A Mass of Li = 370.0 g  Molar mass of Li = 6.94 g/mol

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.