Find the mass of Zn metal deposited at the cathode during the passage of 10 amperes current through its salt solution for 10 minutes. [ Molar mass of Zn = 65.4 g mol^ -1 & For the reaction of Zn, mole ratio = 1/2 ]

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Correct answer: B. 2.0 g

Given: Current I = 10 A Time t = 10 minutes = 10 × 60 = 600 s Molar mass of Zn M = 65.4 g mol^ -1 Valency factor n = 2 (since mole ratio is 1/2 ) Faraday's constant F = 96500 C mol^ -1 According to Faraday's first law of electrolysis: m = (M)/(nF) It Substituting the values: m = (65.4)/(2 × 96500) × 10 × 600 m = (65.4 × 6000)/(193000) m = (392.4)/(193) 2.03 g The closest value is 2.0 g. Answer: 2.0 g

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