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Calculate the equilibrium constant for t...

Calculate the equilibrium constant for the reaction
`Fe^(2+)+Ce^(4+)hArrFe^(3+)+Ce^(3+)`
`(Given E_(Ce^(4+)//Ce^(3+))^@=1.44V and E_(Fe^(3+)//Fe^(2+))^@=0.68V)`

Text Solution

Verified by Experts

`E_(cell)^@=0.059/1logK_C` " " [n=1]
or `E_(cell)^@=E_(Ce^(4+)//Ce^(3+))^@-E_(Fe^(3+)//Fe^(2+))^@=1.44-0.68=0.76V`
`therefore` 0.76=0.059log `K_(C)` or `logK_(C)=0.76/0.059=12.8814`
or `K_(C)=7.6xx10^(12)`
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