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Determine the values of equilibrium constant `(K_C) and DeltaG^o` for the following reaction : |
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Answer» The cell reaction is `Ni(s)+2Ag^+(aq)toNi^(2+)(aq) +2Ag(s)`, `DeltaG^o=-nFE^o` `E^o=1.05V,n=2,f=96500C//"mol"`. `DeltaG^o=-(2mol)xx(96500C//mol)xx(1.05V)`. `=-202650 CV (1CV=1)` `=-202650J` Colculation of K in the from `DeltaG^o`, `DeltaG^o=-202650J,R=8.314J//mol//K`. `T=298k`. `logK=(DeltaG^o)/(2.303RT)=(-202650J)/((2.303)xx(8.314J//mol//K)xx(298K))` `=K=(-202650)/5705.84832=35.51` `or K=0.35xx10^2` |
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