Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If a current of 6.0A and a voltage of 4.5V are used: a) How many hours would it take to completely convert 215mL of 1.25M K2Cr2O7 to elemental chromium? b) How many kilowatt-hours of electrical energy are required to plate 1.00 g of chromium?

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: a) 215 ml  ofb1.25  potassium  means (1.25/1000)×215 = 0.26 mol of potassium dichromate.   From the…

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Given that: Molarity of K2Cr2O7 = 1.25 M Volume of K2Cr2O7 = 215 mL = 0.215 L

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Current = 5 A Voltage = 4.5 V Time = ? Volume = 215 mL = 0.215 L Molarity = 1.19 M

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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.