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Two electrolytic cells, one with AgNO₃ and another with CuSO₄, are connected in **series** and the same current of 5 A is passed for 1 hour. The molar masses of Ag and Cu are 108 and 63.5 g/mol respectively. The ratio of masses of Ag to Cu deposited at their respective cathodes is approximately:
A108 : 31.75 ≈ 3.40 : 1
B1 : 1
C216 : 63.5 ≈ 3.40 : 1
D108 : 63.5 ≈ 1.70 : 1
Answer & Solution
Correct answer: A. 108 : 31.75 ≈ 3.40 : 1
Same charge passes through both. Mass ∝ equivalent weight = M/n. Ag⁺ + e⁻ → Ag (n=1) ⇒ eq.wt = 108. Cu²⁺ + 2e⁻ → Cu (n=2) ⇒ eq.wt = 63.5/2 = 31.75. Ratio mass(Ag) : mass(Cu) = 108 : 31.75 ≈ 3.40 : 1.
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