Plating Eyeglasses: How Long for 0.5g Gold/Copper?

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Homework Help Overview

The discussion revolves around the electroplating process for eyeglasses, specifically focusing on the deposition of 0.5g of gold or copper onto aluminum frames. Participants are exploring the relationship between the amount of material to be plated, the applied voltage, and the time required for the plating process.

Discussion Character

  • Exploratory, Assumption checking, Problem interpretation

Approaches and Questions Raised

  • Participants are attempting to calculate the time required for plating based on the amount of gold and the electrochemical principles involved. Questions arise regarding the correct application of formulas and the impact of voltage on the plating process.

Discussion Status

The discussion is ongoing, with participants questioning the assumptions about the applied voltage and its role in the plating process. Some have provided calculations while others seek clarification on the relationship between voltage, current, and plating time.

Contextual Notes

There is a noted lack of information regarding the specific applied voltage, which is critical for determining the current and thus the plating time. Participants are also examining the implications of using different metals for plating.

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"bar of gold or copper placed in acidic solution, attached via battery to item to be plated. Eyeglasses plated placed in solution, voltage applied to create electrolytic cell, which plates material."
1. Total amount of gold to deposit on glasses made of aluminum = 0.5g. How long should the plating process be performed to deposit this amount of gold?
2. If the glasses are plated with copper instead of gold...
A) Reaction require lower V, proceed at same speed for equal current
B) Reaction require lower V, but proceed more quickly
C) Reaction require same voltage but proceed slowly for equal current

Reduction potentials:
Au3+ + 3e --> Au 1.5V
Cu2+ + 2e --> Cu 0.34V
Al3+ + 3e --> Al 1.66V

Attempts:
1. 0.5g x (1mol/197gAu) x (3e-/1mole) x (96487C/mole) x 1s/C = ~730s
However, answer is 73s because the last term they did is 1s/10C. How come?

2. I was thinking that the reaction would require a higher voltage since the difference between the reduction potential of Al and Cu is greater than the difference between Al and Au.

Thank you.
 
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What is the applied voltage? and that should explain the /[C] question
 
The question actually doesn't mention anything about the applied voltage... at least I don't see it.
 
It only says "A voltage is applied to create an electrolytic cell, which plates the material onto the eyeglass frames."
 
The amount of plating depends on how much current is flowing which depends on the applied voltage(source). You need more information.
 

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