How much time is required to deposit 1 × 10-3 cm thick layer of silver (density is 1.05 g cm-3) on a surface of area 100 cm2 by passing a current of 5 A through AgNO3 solution?

Question

How much time is required to deposit 1 × 10-3 cm thick layer of silver (density is 1.05 g cm-3) on a surface of area 100 cm2 by passing a current of 5 A through AgNO3 solution? (A) 125 s (B) 115 s (C) 18.7 s (D) 27.25 s

Tardigrade Admin · Accepted Answer

Mass of Ag in coated layer = V × d =1×10-3×100×1.05 =0.105 g W=(I× t× Eq.wt./96500) t=(W×96500/I× Eq. wt.) =(0.105×96500/5×108) =18.7 s

Q. How much time is required to deposit $1 \times 1 0^{- 3} c m$ thick layer of silver (density is $1.05 g c m^{- 3}$ ) on a surface of area $100 c m^{2}$ by passing a current of $5 A$ through $A g N O_{3}$ solution?

$125 s$

$115 s$

$18.7 s$

$27.25 s$

Mass of $A g$ in coated layer $= V \times d$
$= 1 \times 1 0^{- 3} \times 100 \times 1.05$
$= 0.105 g$
$W = \frac{I \times t \times Eq . wt .}{96500}$
$t = \frac{W \times 96500}{I \times Eq . wt .}$
$= \frac{0.105 \times 96500}{5 \times 108}$
$= 18.7 s$

Q. How much time is required to deposit 1×10−3cm thick layer of silver (density is 1.05gcm−3) on a surface of area 100cm2 by passing a current of 5A through AgNO3​ solution?

125s

115s

18.7s

27.25s