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Calculate the standard cell potential (i...

Calculate the standard cell potential (in V) of the cell in which following reaction takes place:
` Fe ^( 2 + ) ( aq ) + A g^ + ( aq ) to Fe ^( 3 + ) ( aq ) + Ag (s ) `
Given that ` E _ (Ag ^ + // Ag ) ^ 0 = x V , E _ ( Fe^( 2+ ) // Fe ) ^0 = yV , E _ (Fe^(3+)//F e )^0 = z V `

Text Solution

Verified by Experts

`E_(cell)^(Theta) = E_(("cathode"))^(Theta) - E_((anode))^(Theta)`
`therefore = 0.80 - 0.77 = + 0.03 V`
`Delta_(r) G^(Theta) = - n F E_(cell)^(Theta)`
`= - 1 xx 96500 xx 0.03`
`= -2896500 CV mol^(-1)`
`= - 289500 J mol^(-1)`
`= -289.5 kJ mol^(-1)`
log `K_(c) = ( n E_(cell)^(Theta))/(0.059)`
`= (1xx 0.03)/(0.059) = 0.508`
`K_(c) = 3.22`
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