1.

Calculate the standard cell potential of the galvanic cell in which the following reaction takes place: 2Cr(s)+3Cd^(2+)(aq)to2Cr^(3+)(aq)+3Cd(s) Also calcuate the triangle_(r)G^(ɵ) value of the reaction (given E_(cr^(3+)//Cr)^(ɵ)=-0.74V,E_(Cd^(3+)//Cd)^(ɵ)=-0.40V and F=96500Cmol^(-1)

Answer»

Solution :`E_("cell")=E_("cathode")^(@)-E_("anode")^(@)`
`=-.40-(-0.74)=0.34V`
`DeltaG^(@)=-nFE_("cell")^(@)=-6xx96500xx0.34=-196860`
`=-"196868 J mol"^(-1)=-"196.86 kJ/mol"`
`-DeltaG^(@)=2.303" RT log K"_(c)`
`196860=2.303xx8.314xx"298 log K"_(c)`
`"ORLOG K"_(c)=34.5014`
`K_(c)="antilog 34.5014"=3.192xx10^(34)`


Discussion

No Comment Found

Related InterviewSolutions