Calculate `Delta_(r)G^(@)` and log `K_(c)` for the following reaction at 298 K.
`2Cr_((s))+Cd_((aq))^(3+)+33Cd_((s)){Given :E^(@)""_(Cell")=+0.34V,IF=96500Cmol^(-1)]`

Explanation

`2Cr_((s))+3Cd_((aq))^(3+)+3Cd(s)`
`E^(@)cell =0.34V, IF=96500C//mol.`
`DeltaG^(@)=-nFE^(@)cell`
For this reaction , n = 6
`[{:(2Crto2Cr^(3+)+6e^(-)),(3Cd^(3+)+6e^(-)to3Cd):}]`
`DeltaG =-6 xx96500xx0.34`
`DeltaG=-196860J//molk_(c)`
`DeltaG=-2.303RT log k_(c)`
`logk_(c)""(-DeltaG)/(2.303xx8.314xx298)`
`logk_(c)=(+196860)/(2.303xx8.314xx298)`
`log k_(c)=34.5014`