Electrochemistry - Result Question 36
####35. How many grams of silver could be plated out on a serving tray by electrolysis of a solution containing silver in +1 oxidation state for a period of $8.0 h$ at a current of $8.46 A$ ? What is the area of the tray, if the thickness of the silver plating is $0.00254 cm$ ? Density of silver is $10.5 g / cm^{3}$.
(1997, 3M)
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Solution:
- Coulombs passed $=8.46 \times 8 \times 60 \times 60=243648 C$
Number of Faraday’s passed $=\frac{243648}{96500}=2.52$
Weight of $Cu$ plated $=2.52 \times \frac{63.5}{2} g=80.01 g$
Volume of $Cu$ plated $=\frac{80.01}{10.5}=7.62 cm^{3}$
$\Rightarrow$ Area plated out $=\frac{7.62}{0.00254}=3000 cm^{2}$
