Question

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.

Name: a current of 0452 amps is passed through an electrolytic cell containing molten cacl2 for 150 hrs write the electrode reactions at both the anode and the cathode electrodes and calculate the 23548
Uploaded: 2023-04-26T19:43:01-08:00
Duration: 3 min 1 s
Channel: David Collins
Description: a current of 0452 amps is passed through an electrolytic cell containing molten cacl2 for 150 hrs write the electrode reactions at both the anode and the cathode electrodes and calculate the 23548

          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.

Added by Albert S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

04/26/2023

Step 1

At the cathode, the reduction half-reaction occurs. Calcium ions (Ca²⁺) gain electrons to form calcium metal (Ca): $$\text{Cathode: } \mathrm{Ca^{2+} + 2e^- \rightarrow Ca}$$ At the anode, the oxidation half-reaction occurs. Chloride ions (Cl⁻) lose electrons Show more…

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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.