Calculate `DeltaG^(@)` and log `K_(c)` for the following reaction at 298 K : `2Al(s)+3Cu^(2+)(aq)rarr2Al^(3+)(aq)+3Cu(s)` Given `E_(cell)^(@)`=2.02 V
Calculate `DeltaG^(@)` and log `K_(c)` for the following reaction at 298 K :
`2Al(s)+3Cu^(2+)(aq)rarr2Al^(3+)(aq)+3Cu(s)`
Given `E_(cell)^(@)`=2.02 V
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(i) Calculate of `DeltaG^(@)` for the reaction :
`2Al(s)+3Cu^(2+)(aq)rarr2Al^(3+)(aq)+3Cu(s)`
`DeltaG^(@)=-nFE_(cell)^(@)`
`DeltaG^(@)=(-6)xx(96500" C mol"^(-1))xx(2.02 V)=-1169580" C V mol"^(-1)`
`=-1169580 " J mol"^(-1)=-1169.580 " kJ mol"^(-1)`
(ii) Calculate of equilibrium constant `(K_(c))` for the reaction
log `K_(c)=(nE_(cell)^(@))/((0.0591 V))=(6xx(2.02 V))/((0.0591 V))=205`
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