Respuesta :
Answer:
Max. work done in 60 g of copper plated out is 200472.14 J
Explanation:
Given cell reaction is:
[tex]Zn(s)+Cu^{2+} \rightarrow Zn^{2+}+Cu(s)[/tex]
Standard reduction potential of Zn electrode ([tex]E_{Zn^{2+}/Zn}[/tex]) is 0.763 V.
Standard reduction potential of Cu electrode ([tex]E_{Cu^{2+}/Cu}[/tex]) is -0.337 V.
Copper acts as cathode and Zinc acts as anode.
Cell potential (E) = E° cathode - E° anode
= 0.763 - (-0.337)
= 1.10 V
formula for the work done is as follows:
[tex]W_{max}=-nFE[/tex]
Here, n is no. of electron involved in the reaction.
F(Faraday's constant) = 96500
In the given reaction, n = 2
[tex]W_{max}=-nFE\\=-2 \times\ 96500 \times 1.10\\=-212300\ J/mol[/tex]
Therefore, 212300 J work is done by reducting 1 mol of copper.
Copper given is 60 g.
Molecular mass of copper is 63.54 g/mol.
[tex]No.\ of\ mol = \frac{60\ g}{63.54\ g/mol}[/tex]
Max. work done in 60 g of copper plated out is:
[tex]W_{max}=212300\ J/mol \times \frac{60\ g}{63.54\ g/mol} \\=200472.14\ J[/tex]
