Question

In a copper electrolysis tank what mass of copper is deposited by a current of 10ka in minutes.

Answer 1

Final Answer: 3.29t grams
Let time = t (in secs)

Steps:
1) By Faraday's Law of Electrolysis,
W = ZQ = (M/nF)* Q
where
Z = Electrochemical equivalent of chemical species =M/nF = Molar Mass /nF
1F = 96,500C
n= moles of electron gained /losed per mole of species.

Q = Charge passed during production/use of Z

2) M = 63.5g
I = 10 kA = 10 * 10^3 = 10^4A
Q = 10^4*t C
Assuming Reaction is :
Cu2+ is from Copper Sulphate solution
Cu(2+) + 2e -------> Cu (s)
n= 2
$w = \frac{63.5}{2 \times 96500} \times {10}^{4} \times t \\ = > \frac{63.5}{2 \times 965} \times 100 \times t \\ = > 3.29t \: \: \: grams$
where t is in seconds.
Here, substitute value of time in seconds to get mass of Copper produced.