Write the cell formulation and calculate the standard cell potential of the galvanic cell in operation of which the reaction taking place is: `2Cr(s)+3Cd^(2+)(aq)to2Cr^(3+)(aq)+3Cd(s)` Calculate `Delta_(r)G^(@)` for the above reaction. (Given: `E_(Cr^(3+)//Cr)^(@)=-0.74V,E_(Cd^(2+)//Cd)^(@)=-0.40V,F=96500" "C" "mol^(-1)`)

Write the cell formulation and calculate the standard cell potential o

1.	Write the cell formulation and calculate the standard cell potential of the galvanic cell in operation of which the reaction taking place is: `2Cr(s)+3Cd^(2+)(aq)to2Cr^(3+)(aq)+3Cd(s)` Calculate `Delta_(r)G^(@)` for the above reaction. (Given: `E_(Cr^(3+)//Cr)^(@)=-0.74V,E_(Cd^(2+)//Cd)^(@)=-0.40V,F=96500" "C" "mol^(-1)`)
Answer» Correct Answer - `+0.34V,-196.86kJ" "mol^(-1)` `Cr(s)\|Cr^(3+)(aq)\|\|Cd^(2+)(aq)\|Cd(s)` `2Crto2Cr^(3+)+6e^(-)` or `3Cd^(2+)+6e^(-)to3Cd`. Hence, n=6 `E_(cell)^(@)=-0.40-(-0.74)=+0.34V,Delta_(r)G^(@)=-nFE_(cell)^(@)`

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