How long would it take to electroplate a flute with 28.3 g of silver at a constant current of 2.0 amps using AgNO₃?

Question

Quizplus · Accepted Answer

The correct formula for silver nitrate is likely intended to be AgNO3, but the provided formula seems to be a typographical error. To calculate the time required for electroplating, we use Faraday's laws of electrolysis. The molar mass of silver (Ag) is 107.8682 g/mol, and the charge required to reduce one mole of Ag+ ions is 96,485 C (Coulombs) because silver has a valency of 1. First, calculate the moles of silver to be plated:$$ \text{Moles of Ag} = \frac{28.3 \text{ g}}{107.8682 \text{ g/mol}} $$$$ \text{Moles of Ag} = 0.2624 \text{ mol} $$Next, calculate the total charge needed:$$ \text{Charge} = \text{Moles of Ag} \times \text{Charge per mole of Ag} $$$$ \text{Charge} = 0.2624 \text{ mol} \times 96,485 \text{ C/mol} $$$$ \text{Charge} = 25,336 \text{ C} $$Finally, calculate the time required using the current:$$ \text{Time} = \frac{\text{Charge}}{\text{Current}} $$$$ \text{Time} = \frac{25,336 \text{ C}}{2.0 \text{ A}} $$$$ \text{Time} = 12,668 \text{ s} $$To convert seconds to minutes:$$ \text{Time} = \frac{12,668 \text{ s}}{60 \text{ s/min}} $$$$ \text{Time} \approx 211 \text{ min} $$Therefore, it would take approximately 211 minutes to electroplate the flute with 28.3 g of silver at a constant current of 2.0 amps.

How Long Would It Take to Electroplate a Flute with 28.3