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Predict whether the following reactions occur under standard state conditions : (a) Oxidationof 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 |
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Answer» Solution :(a) SINCE THESTANDARD reduction potentialof `Cl_(2(g))` ishigher`(E_(cl^(2+)//cl^(-0))^(0) - = 1.36V) `than thatof `Ag,(E_(Ag^(2+)//Ag)^(0) = 0.8V)`,chlorine will oxidise `Ag_((S))` to `Ag^(+)` . The redox reactionwill be , `2Ag_((s)) + Cl_((2)) to2Ag^(+) + 2Cl_((aq))^(-)` (B) Sincethestandardreductionpotential of Auis higher`(E_(Cl^(2+)//Cl^(-))^(0) = - 1.4V)` thanthat of `Fe^(3+)`, Fe^(2+)`couple`(E_(Fe^(3+),Fe^(2+))^(0) = 0.77V)` , Auwillnot reduce `Fe^(3+)`, to `Fe^(2+)` but Au can oxidise `Fe^(2+)` to `Fe^(3+)` sinceAu has moretendency to accpet electrons. |
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