Electrolysis (1)

Chemistry Level 3

Solid silver sulfate (Credit: Google Images) Solid silver sulfate (Credit: Google Images)

During the electrolysis of an aqueous solution of A g X 2 S O X 4 \ce {Ag2SO4} with platinum electrodes a time-dependent current I ( t ) = 2 t 3 + 1 I(t) = 2t^3 +1 (where t t is in seconds) was supplied under a constant efficiency of 75 75 % for 4 4 seconds under STP conditions. Find the weight of the discharged metal at cathode (in grams).

Details: Use Faraday's constant F = 96500 C mol − 1 F = 96500 \text{ C mol}^{-1} and weight of A g = 108 gm \ce{Ag} = 108 \text{ gm} .


The answer is 0.11.

Tapas Mazumdar by Tapas Mazumdar , 20, India

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1 solution

Suhas Sheikh
Jul 6, 2018

Find total charge passed by integrating I(t),w.r.t time Then multiply this charge with the efficiency of the current (Being a constant,it doesn't make a difference in the integral) Then find mols of electrons corresponding to the charge This gives you the mols of At deposited at cathode Multiplying by 108g yields the desired answer

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