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Question: How much time is required to deposit \(1 \times 10^{- 3}\)cm thick layer of silver (density is \(1.0...

How much time is required to deposit 1×10−31 \times 10^{- 3}cm thick layer of silver (density is 1.05gcm31.05gcm^{3}) on a surface of area 100cm2100cm^{2} by passing a current of 5 A through AgNO3AgNO_{3}solution?

A

125 s

B

115 s

C

18.7s18.7s

D

27.25s27.25s

Answer

18.7s18.7s

Explanation

Solution

Mass of Ag in coated layer = V × d

=1×10−3×100×1.05=0.105g= 1 \times 10^{- 3} \times 100 \times 1.05 = 0.105g

W=I×t×Eq.wt96500W = \frac{I \times t \times Eq.wt}{96500}

t=W×96500I×Eq.wt=0.105×965005×108=18.7st = \frac{W \times 96500}{I \times Eq.wt} = \frac{0.105 \times 96500}{5 \times 108} = 18.7s