Represent the cell in which the following reaction takes place

Mg(s) + 2Ag+(0.0001M) ------ Mg2+(0.130M) + 2Ag(s)

Calculate its E( cell) if E0 (cell)=3.17 V.

Dear Student,

The cell will be represented as:

Now, for determination of Ecell , we follow as:

Ecell = E0(cell)  - 0.059/ n log [Mg+2 ]/ [Ag+ ]2 

Her, no. of electrons involved , n =2 

So, Ecell = E0(cell)  - (0.059/ 2) log [Mg+2 ]/ [Ag+ ]2 

Ecell = 3.17 - 0.059/ 2 log [0.130 ]/ [0.0001 ]2  =3.17 - 0.0295log 13 x 106 = 3.17-0.0295(7.113) = 2.96 V

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