The same current is passed for the same time through solutions of AgNO3 and CuSO4 connected in series. How much silver will be deposited if 1.0 g of copper is produced?
[Cu = 63.5, S = 32, O = 16, Ag = 108, N = 14]
[Cu = 63.5, S = 32, O = 16, Ag = 108, N = 14]
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Correct Answer: Option B
Explanation:
From Faraday;s second law of electrolysis
\(\frac{\text{Mass of silver deposited}}{\text{Mass of copper deposited}}\) = \(\frac{\text{Equivalent mass of silver}}{\text{Equivalent mass of copper}}\)
\(\frac{\text{Mass of silver deposited}}{1.0g}\) = \(\frac{108}{63.5}\)
= 31.75g
Copper is devalent = Cu2+
Mass of silver deposited = \(\frac{108g}{31.75g}\)
= 3.30g
From Faraday;s second law of electrolysis
\(\frac{\text{Mass of silver deposited}}{\text{Mass of copper deposited}}\) = \(\frac{\text{Equivalent mass of silver}}{\text{Equivalent mass of copper}}\)
\(\frac{\text{Mass of silver deposited}}{1.0g}\) = \(\frac{108}{63.5}\)
= 31.75g
Copper is devalent = Cu2+
Mass of silver deposited = \(\frac{108g}{31.75g}\)
= 3.30g