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Question

A solution of CuSO4 is electrolysed for 10 minutes with a current of 1.5 amperes. what is the mass of copper deposited at the cathode?


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Solution

Step 1: Given data

Time(t)=10min=10×60=600sec

Current(A)=1.5A

Step 2: Framing the reaction

From the above question, we can form the reaction at cathode as,

Cu2+(aq)Copperions+2e-ElectronsCu(s)Copper

Thus 2 electrons are transferred here.

Step 3: Finding the mass of copper

The mass of copper we know is 63.5gmol-1

W know that,

Charge=time×currentCharge=600×1.5Charge=900C

Now, Mass of copper deposited

=Molarmass×Chargeelectronstransferred×Faradaysconstant=63.5×9002×96500=57150193000=0.296g

Therefore, the mass of copper deposited at the cathode is 0.296g


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