Department of Pre-University Education, KarnatakaPUC Karnataka Science Class 12
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Calculate e.m.f. and ∆G for the following cell - Chemistry

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Calculate e.m.f. and ∆G for the following cell:

Mg (s) |Mg2+ (0.001M) || Cu2+ (0.0001M) | Cu (s)

`"Given :" E_((Mg^(2+)"/"Mg))^0=−2.37 V, E_((Cu^(2+)"/"Cu))^0=+0.34 V.`

 

 
 
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Solution

 
 

For the given cell representation, the cell reaction will be

Mg(s) + Cu2+(0.0001 M) → Mg2+(0.001 M) + Cu(s)

The standard emf of the cell will be given by

 

         = 0.34 - (-2.37)

         = 2.71 V

The Nernst equation for the cell reaction at 25 ºC will be

`E_(Cell)=E_(Cell)^@-(0.059/n)"log"([Mg^(2+)])/([Cu^(2+)])`

        `=2.71-0.059/2"log"0.001/0.0001`

        `=2.71-0.02955(log10)`

        `=2.71-0.02955(1)`

        `=2.68045V~~2.68V`

 We know

nFEcell

     =2×96500×2.68

     =517240 J mol1

     =517.24 kJ mol1

Concept: Galvanic Cells - Introduction
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