What is the equation for Faraday's law of electrolysis?

Click For Summary
SUMMARY

The discussion centers on calculating the current in an electrolytic cell where 3.00 x 10-3 kg of gold is deposited over 2.62 hours. The relevant equations include delta Q/delta T and n*q*vd*A, where n represents moles, q is the charge, vd is the drift speed, and A is the cross-sectional area. The key to solving the problem lies in applying Faraday's law of electrolysis, which relates the amount of substance deposited to the charge passed through the cell. The hint provided emphasizes the relationship between the number of electrons per atom and moles of gold.

PREREQUISITES
  • Understanding of Faraday's law of electrolysis
  • Knowledge of charge, moles, and drift speed in electrochemistry
  • Familiarity with the concept of current and its calculation
  • Basic principles of electrolytic cells
NEXT STEPS
  • Study the derivation of Faraday's law of electrolysis
  • Learn how to calculate current using the formula I = Q/t
  • Explore the relationship between moles and electrons in electrochemical reactions
  • Investigate the effects of different variables on the efficiency of electrolytic cells
USEFUL FOR

This discussion is beneficial for students studying electrochemistry, particularly those tackling problems related to electrolytic cells and Faraday's law. It is also useful for educators and anyone involved in practical applications of electrolysis in chemistry.

J89
Messages
29
Reaction score
0

Homework Statement


If 3.00 10-3 kg of gold is deposited on the negative electrode of an electrolytic cell in a period of 2.62 h, what is the current in the cell during that period? Assume the gold ions carry one elementary unit of positive charge.




Homework Equations


delta Q/delta T
n*q*vd*A: n = moles, q=charge, vd=drift speed and A= cross sectional area of conductor.



The Attempt at a Solution



I'm having a bit trouble starting this because I think we have to derive an equation since we only have mass and the time, and nothing else given. I tried to put the two equations posted together, but it did not look right nor make sense. Can someone give a hint on how to start this?
 
Physics news on Phys.org
Google Faraday's law of electrolysis.

But with some thinking you should be able to solve it on your own. There is one electron per atom - how many electrons per mole?
 
Last edited by a moderator:

Similar threads

Galvanic Cell Changes: Copper Deposition on X
  • · Replies 2 ·
Replies
2
Views
2K
High School What is the difference between N = Q/nF and m = Z*I*t in electrolysis?
  • · Replies 4 ·
Replies
4
Views
4K
What is the mass of H2 and O2 produced water electrolysis?
  • · Replies 3 ·
Replies
3
Views
3K
What Is the Cell Potential When Pb Electrode Mass Changes?
  • · Replies 10 ·
Replies
10
Views
4K
Does Faraday's Law of Electrolysis Measure Mass Change at One Electrode or Both?
  • · Replies 2 ·
Replies
2
Views
7K
Electrolysis of water and actual electrode potential.
  • · Replies 3 ·
Replies
3
Views
2K
How Does Ion Charge Affect Mass Deposition in Electrolysis?
  • · Replies 66 ·
3
Replies
66
Views
16K
Undergrad Direct and alternating current, a personal approach to understand them
  • · Replies 1 ·
Replies
1
Views
2K
How many moles of gold are deposited on the electrode in 10.98 hours?
  • · Replies 4 ·
Replies
4
Views
2K
How Does Faraday's Law of Electrolysis Apply to Reversible Reactions?
  • · Replies 12 ·
Replies
12
Views
5K