Calculate the amount of zinc deposited at the cathode when 3 amperes current is passed through the electrolyte for 2 minutes. Also, calculate the equivalent weight and oxidation state of the other metal if 0.245 grams of the metal is deposited by the same quantity of the electricity.
(Atomic weight of metal = 197 g/mole)

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Solution

$I = 3 a m p e r e s t = 2 m i n u t e s w = Z I t = \frac{65.3}{2 \times 96500} \times 3 \times 2 \times 60 = 0.121 g$
For other metal $w = 0.245 g 0.245 = \frac{e q . w t}{96500} \times 3 \times 60 \times 2 e q . w t = 65.40 g / e q . \frac{m o l a r m a s s}{o x i d a t i o n s t a t e} = 65.40 3 = O . S$

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I=3amperest=2minutesw=ZIt=65.32×96500×3×2×60=0.121gFor other metal w=0.245g0.245=eq.wt96500×3×60×2eq.wt=65.40g/eq.molarmassoxidationstate=65.403=O.S