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The apparatus in the image was set up. 1 mol of copper II sulfate was used in the...

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jordanf369 | Student | eNoter

Posted July 3, 2013 at 6:37 AM via web

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The apparatus in the image was set up.


1 mol of copper II sulfate was used in the electroplating. The switch on the power source was turned on and simultaneously the timer was started. At 20 minutes the reaction was stopped (the switch turned off).

How much copper was deposited on the carbon cathode? (Is it even possible to figure out the theoretical value?)


Thanks

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justaguide | College Teacher | (Level 2) Distinguished Educator

Posted July 3, 2013 at 6:49 AM (Answer #1)

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The figure shows a set up for electroplating with the anode and cathode, both of which are made of copper dipped in a copper(2) sulfate bath. A potential difference of 2 V is created between the electrodes by including a cell.

The potential difference between the two electrodes results in copper from the anode getting converted to copper ions an moving towards the cathode through the solution they are dipped in.

There is no information provided about the resistance of the components involved in the circuit. As a result the current flowing through the circuit cannot be determined. This makes it impossible to determine the mass of copper deposited on the cathode.

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