Find the amount of silver liberated at cathode if 0.500 A of current is passed through AgNO3 electrolyte for 1 hour. Atomic weight of silver is 107.9 g mol–1.


Given


Equivalent mass of silver EAg = 107.9 g


Current passed = 0.005 A


We know


1 F (faraday) is 1 mol of electrons



⇒1 F = one electron (1.602 x 10-19) ×Avogadro's number (6.022 x 1023)


= 96,500 C of charge



⇒ Amount of charge required is 12 times of 6.023 × 1023 =


= 96500 C of charge



The Electrochemical equivalent of silver,



Where


E is the equivalent mass of silver


Agf is the amount of charge




Using the formula, from faraday’s law of electrolysis –



where,


m = the mass of the substance deposited on the electrode


z=electrochemical equivalence


i=current passing


t=time taken


we get:









So, 2.01 g of silver is liberated on electrode.


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