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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))

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SOLUTION :`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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