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Sagot :
Mass of copper would be=92.46 g
I = Current = 19.5 A
t = 4 hours =4×60×60=14400 s
F = Faraday constant = 96485.33 C/mol
Molar mass of copper = 63.546 g/mol
A charge is given by
Q=19.5×14400=280880 C
Moles of electrons are given by Q/F=280880/96485.33=2.91 mol
Moles of copper is=1/2×2.91=1.455 mol
Mass of copper would be=1.455×63.546=92.46 g
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#4206.
The mass of Copper electroplated is 68.76 g
What is electroplating?
The process of plating a metal onto another is known as electroplating.
It is often used to prevent corrosion of metal or for the decorative purposes
In this process, electric current is passed through an aqueous solution containing dissolved cations.
The dissolved cations are reduced developing a thin metal coating on the electrode.
At cathode,
[tex]Cu^{2+}(aq) + 2e^-\rightarrow Cu(s)[/tex]
Current, I = 14.5 A
Time, t = 4 hrs = 4×60×60 = 14400 sec
Charge, q = It = 14.5×14400= 208800 C
Copper metal deposited by 2×96487 C = 63.55 g
Copper metal deposited by 208800 C = [tex]\frac{63.55 \times208800}{2\times96487}[/tex]
= 68.76g
Hence, The mass of Copper electroplated is 68.76 g
Learn more about electroplating:
https://brainly.com/question/22104403
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