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Electrochemistry

Question

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A current of 1.50 amp passed through an electrolytic cell containing AgNO₃solution with inert electrodes. The weight of Ag deposited was 1.50 g. How long did the current flow?

Solution

Ag + + e^{-} \to Ag 1 mol 1 mol (or 108 g)

108 g of silver needs = 1 Faraday
= 96500 coulombs

∴

1.50 g of silver needs =

\frac{96500 \times 1.50}{108}

= 1340.3 coulomb
But Q = current x time
1340.3 = 1.5A x time (in sec)
Time for which current is passed =

\frac{1340.3}{1.5}

= 893.5 sec = 14.9 min

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