What quantity of current is required to deposit 2.4g of copper in a period of...
CHEMISTRY
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What quantity of current is required to deposit 2.4g of copper in a period of 750 seconds during an electrolytic deposition process? [Cu 64, IF = 96500C mol?1]
- A) 9.65A
- B) 10.81A
- C) 12.33A
- D) 15.54A
Correct Answer: A) 9.65A
Explanation
\( n = \frac{m}{M} = \frac{2.4}{64} = 0.0375 \)
1 mole of electron = 1F = 96500
\( Cu ^{2+} \) = 2 moles of electron = 2F =96500 x 2 = 193000
Q = It \( \therefore I = \frac{Q}{t} \)
Q = 193000 x 0.0375 = 7237.5
\( I = \frac{7237.5}{750} = 9.65A\)
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