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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?

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?

Grade:8

4 Answers

Gaurav
askIITians Faculty 164 Points
9 years ago
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Akash
15 Points
5 years ago
estimate the mass of copper metal produced during passage of 5A current through CuSO4 solutions for 100 min (the molar mass of Cu is 63.5g/mol.)
Punit
15 Points
4 years ago
Here,Charge available Q is,
Q=5*6000=30000C
But as we know,that here in this question
2*96500C=63.5g
1C=63.5/2*96500
30000C= 63.5*30000/2*96500
Rishi Sharma
askIITians Faculty 646 Points
3 years ago
Hello Prasanjeet,
The solution is as follows
The cathodic reaction is
Cu2+ + 2e- → Cu
I = 1.5 A
t = 10 min = 10*60 = 600 sec
reaction states that 2 * 96500 C requires to deposit 63.5 g of Cu at cathode
for 900 C will deposit = 63.5 * 900 / (2 * 96500 )
= 0.296 g

Thanks
I hope above solution will clear your all doubts.
Please feel free to post and ask as much doubts as possible.
All the best.





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