If a current of 724.2 mA is passed through an electrochemical cell for 48.32 min

Question

If a current of 724.2 mA is passed through an electrochemical cell for 48.32 minutes, what charge, in coulombs, is passed through the cell? Charge passed through the cell = ?coulombs Suppose that the electrochemical cell consists of two copper electrodes immersed in a copper(II) sulfate solution. At which electrode, anode or cathode, does oxidation occur? The oxidation occurs at the ? Do you expect that this electrode will increase or decrease in mass as the electrolysis proceeds? The mass of the electrode will ? Calculate the change in the mass of copper at the anode or cathode if the charge calculated above is passed through the cell described. Enter your answer as a positive quantity in mg. Mass change at the electrode = ? mg

Explanation / Answer

1) Charge in coulombs = i (amp) x t (sec) = 0.7777 x 27.09 x 60 = 1264.07 C

2) The oxidation occurs at the Anode.

3) The mass of the electrode will decrease.

4) w = (E/F) x i x t = (31.7/96500) x 1264.07 = 0.415 g = 415 mg

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