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How long would it take to deposit 0.08g of copper from CuCl\(_2\) solution by passing...

Chemistry
JAMB 2007

How long would it take to deposit 0.08g of copper from CuCl\(_2\) solution by passing a current of 0.5A?
[Cu = 64, 1F = 96500 C mol-1]

  • A. 6 mins
  • B. 8 mins
  • C. 24 mins
  • D. 48 mins
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Correct Answer: Option B
Explanation

Cu\(^{2+}\) + 2e- → Cu(s)
2 x 96500C deposits 64g of Cu
x quantity of electricity will deposit 0.08g
x = (2 x 96500 x 0.08)/64 =241.25 coulomb.
Q = It
241.25 = 0.5t
t = 241.25/60 = 8 mins

There is an explanation video available below.


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Explanation Video

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