JAMB - Chemistry (2007 - No. 17)
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]
[Cu = 64, 1F = 96500 C mol-1]
6 mins
8 mins
24 mins
48 mins
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
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
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