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1 year ago

What mass of cu(s)cu(s) is electroplated by running 14. 5 aa of current through a cu2 (aq)cu2 (aq) solution for 4. 00 hh?

Chemistry

2 answers:

AfilCa [17]1 year ago

7 0

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

Learn more about mass here brainly.com/question/19600926

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galina1969 [7]1 year ago

4 0

The mass of Copper electroplated is 68.76 g

<h3>What is electroplating?</h3>

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,

$Cu^{2+}(aq) + 2e^-\rightarrow Cu(s)$

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 = $\frac{63.55 \times208800}{2\times96487}$

= 68.76g

Hence, The mass of Copper electroplated is 68.76 g

Learn more about electroplating:

brainly.com/question/22104403

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