How many grams of silver could be plated out on a serving tray by electrolysis of solution containing silver in +1 oxidation state for a period of 8 hours at a current of 8.46 ampers. What is the area of the tray if the thickness of the silver plating is 0.00254 cm? Density of silver is 10.5 g cm3 .

Question

How many grams of silver could be plated out on a serving tray by electrolysis of solution containing silver in +1 oxidation state for a period of 8 hours at a current of 8.46 ampers. What is the area of the tray if the thickness of the silver plating is 0.00254 cm? Density of silver is 10.5 g cm3 . (A) 1.02× 104cm2 (B) 102× 104cm2 (C) 10.2× 104cm2 (D) None

Tardigrade Admin · Accepted Answer

W=(E C t/F) =(107.8 × 8.46 × 8 × 60 × 60/96500)=272.178 text g Volume of silver =(w t ./D e n s i t y) =(272.178/10.5)=25.9 text ml Surface area =(V o l u m e/T h i c k n e s s) =(25.95/0.00254) =1.02× 104cm2

$1.02 \times 1 0^{4} c m^{2}$

$102 \times 1 0^{4} c m^{2}$

$10.2 \times 1 0^{4} c m^{2}$

None

$W = \frac{ECt}{F}$
$= \frac{107.8 \times 8.46 \times 8 \times 60 \times 60}{96500} = 272.178 g$
Volume of silver $= \frac{wt .}{De n s i t y}$
$= \frac{272.178}{10.5} = 25.9 ml$
Surface area $= \frac{V o l u m e}{T hi c kn ess}$
$= \frac{25.95}{0.00254}$
$= 1.02 \times 1 0^{4} c m^{2}$

1.02×104cm2

102×104cm2

10.2×104cm2

None

W=FECt​ =96500107.8×8.46×8×60×60​=272.178 g Volume of silver =Densitywt.​ =10.5272.178​=25.9 ml Surface area =ThicknessVolume​ =0.0025425.95​ =1.02×104cm2

$1.02 \times 1 0^{4} c m^{2}$

$102 \times 1 0^{4} c m^{2}$

$10.2 \times 1 0^{4} c m^{2}$

$W = \frac{ECt}{F}$
$= \frac{107.8 \times 8.46 \times 8 \times 60 \times 60}{96500} = 272.178 g$
Volume of silver $= \frac{wt .}{De n s i t y}$
$= \frac{272.178}{10.5} = 25.9 ml$
Surface area $= \frac{V o l u m e}{T hi c kn ess}$
$= \frac{25.95}{0.00254}$
$= 1.02 \times 1 0^{4} c m^{2}$