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Calculate the standard cell potentials o...

Calculate the standard cell potentials of the galvanic cells in which the following reactions take place :
`Fe^(2+)(aq)+Ag^(+)(aq)rarr Fe^(3+)(aq)+Ag(s)`
Calculate `Delta_(r )G^(0)`, equilibrium constant of the reactions.

Text Solution

Verified by Experts

`E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)=+0.8-0.77=0.03`
`Delta_(r )G^(@)=-nFE_("cell")^(0)=-1xx96500xx0.03=2.895 kJ. mol^(-1)`
Also, `-Delta_(r )G^(@)=2.303` RT log K
log K `=(2.895xx10^(3))/(2.303xx8.314xx298)=0.5074 " " therefore K = 3.216`
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