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]

1.7g

3.4g

6.8g

13. 6 g

Correct answer is B

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

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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]

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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]