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Calculate the cell emf and Delta(r ) G^(...

Calculate the cell emf and `Delta_(r ) G^(@)` for the cell reation at `25^(@)C`.
`Zn(s) | Zn^(@+) ( 0.1 M )|| Cd^(2+) ( 0.01M) | Cd(s)`
Given, `E_(Zn^(2+) //Zn)^(@) = - 0.763V`,
`E_(Cd^(2+) //Cd) ^(@) = - 0.403 V`
1F = 96500 C `"mol"^(-1)`
R = 8.314 `JK^(-1) "mol"^(-1)`],
Find `E_("cell")^(@) = E_("cathode")^(@) - E_("anode")^(@) ` then `Delta _(r ) G^(@)` by using formula, `Delta _(r ) G^(@) = - n FE_("cell")^(@)`

Text Solution

Verified by Experts

The correct Answer is:
`Delta _(r ) G = - 69480 J "mol"^(-1)`
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