Electroplating Zinc onto Copper: Calculating Time Needed

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SUMMARY

The discussion focuses on calculating the time required to electroplate zinc onto a 1.00 mm thick copper sheet, aiming for a zinc thickness of 140 µm. The electroplating process uses divalent zinc ions in an ionic solution and operates at a current of 1.40 A. Key calculations involve using the density of zinc (7140 kg/m³) and Faraday's laws of electrolysis to determine the time needed for the plating process.

PREREQUISITES
  • Understanding of electroplating principles
  • Familiarity with Faraday's laws of electrolysis
  • Knowledge of ionic solutions and charge carriers
  • Basic skills in unit conversion and dimensional analysis
NEXT STEPS
  • Study Faraday's laws of electrolysis in detail
  • Learn about the properties and applications of zinc in electroplating
  • Research the effects of current density on electroplating efficiency
  • Explore the use of different ionic solutions in electroplating processes
USEFUL FOR

This discussion is beneficial for chemistry students, electroplating technicians, and anyone involved in materials science or surface engineering looking to understand the electroplating process and its calculations.

lw1006
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Wow. Can anyone please tell me how to approach this problem?

For a science experiment you need to electroplate zinc onto both sides of a very thin, 1.00 1.00 copper sheet. You want the zinc thickness to be 140 , and you know that the charge carriers in the ionic solution are divalent (charge ) zinc ions. The density of zinc is 7140 .

If the electroplating apparatus operates at 1.40 , how long will it take the zinc to reach the desired thickness?
 
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Why don't you show us how far you got? You know, that thing in the template which somehow is missing from your message.
 


that's the thing. Mastering Physics homework assignments give problems that are not covered in lecture or in the book. That is why I don't even know how to approach this problem, or what formula to use :T
 

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