Question

The standard electrode potential for Deniell cell is `1.1V`. Calculate the standard Gibbs energy for the reaction.
`Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq)+Cu(s)`

Answer 1

`Delta_(r)G^(Ө)=-nFE_((cell))^(Ө)`
n in above equation is 2, `F=96487C" "mol^(-1) and E_((cell))^(Ө)=1.1V`
therefore, `Delta_(r)G^(Ө)=-2xx1.1Vxx96487C" "mol^(-1)`
`=-21227J" "mol^(-1)`
`=-212.27kJ" "mol^(-1)`