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Predict whether the following reactions ...

Predict whether the following reactions occur under standard state conditions :
(a) Oxidation of `Ag_((S))` by `Cl_(2(g)).E_("Ag")^(0) = 0.8V, E_("Cell")^(0) = 1.36V`
(b) Reduction of `Fe^(3+)` to `Fe^(2+)` by `Au_((s))`
`E_(Fe^(3+),Fe^(2+))^(0) = 0.77 V, E_(("Au"))^(2) = 1.4V`

Text Solution

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(a) Since the standard reduction potential of `Cl_(2(g))` is higher `(E_(cl^(2+)//cl^(-0))^(0) - = 1.36V) `than that of `Ag,(E_(Ag^(2+)//Ag)^(0) = 0.8V)`, chlorine will oxidise `Ag_((S))` to `Ag^(+)` .
The redox reaction will be , `2Ag_((s)) + Cl_((2)) to 2Ag^(+) + 2Cl_((aq))^(-)`
(b) Since the standard reduction potential of Au is higher `(E_(Cl^(2+)//Cl^(-))^(0) = - 1.4V)` than that of `Fe^(3+)`, Fe^(2+)` couple `(E_(Fe^(3+),Fe^(2+))^(0) = 0.77V)` , Au will not reduce `Fe^(3+)`, to `Fe^(2+)` but Au can oxidise `Fe^(2+)` to `Fe^(3+)` since Au has more tendency to accpet electrons.
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