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Calculate the standard cell potential of...

Calculate the standard cell potential of the galvanic cell in which the following reaction takes place:
`2Cr(s)+3Cd^(2+)(aq)to2Cr^(3+)(aq)+3Cd(s)`
Also calcuate the `triangle_(r)G^(ɵ)` value of the reaction
(given `E_(cr^(3+)//Cr)^(ɵ)=-0.74V,E_(Cd^(3+)//Cd)^(ɵ)=-0.40V` and `F=96500Cmol^(-1)`

Text Solution

Verified by Experts

`E_("cell")=E_("cathode")^(@)-E_("anode")^(@)`
`=-.40-(-0.74)=0.34V`
`DeltaG^(@)=-nFE_("cell")^(@)=-6xx96500xx0.34=-196860`
`=-"196868 J mol"^(-1)=-"196.86 kJ/mol"`
`-DeltaG^(@)=2.303" RT log K"_(c)`
`196860=2.303xx8.314xx"298 log K"_(c)`
`"Or log K"_(c)=34.5014`
`K_(c)="antilog 34.5014"=3.192xx10^(34)`
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