Show that `E_(Fe^(+3)//Fe^(+2))^(@) =3E_(Fe^(+3)//Fe)^(@)-2E_(Fe^(+2)//Fe)^(@)`

Given that E_(Fe^(2+)//Fe)^(.)=-0.44V,E_(Fe^(3+)//Fe^(2+))^(@)=0.77V if Fe^(2+),Fe^(3+) and Fe solid are kept together then

Assertion (A) Redox couple is the combination of oxidised and reduced form of a substance involved in an oxidation or reduction half cell Reason ( R) In the representation E_(Fe^(-3+)//Fe^(2+))^(ϴ) and E_(Cu^(2+)//Cu)^(ϴ), Fe^(3+)//Fe^(2+) and Cu^(2+)//Cu are redox couples

E_(Fe^(3+)//Fe^(+2))^(0)=+0.77V,E_(Fe^(+3)//Fe)^(0)=0.036V . What is E_(Fe//Fe^(+2))^(0) and is Fe^(+2) stable to disproportionation in aqueous solution under standard conditions

The spontaneous redox reaction //s among the follow is // are (a) 2Fe^(3+)+Fe rarr 3Fe^(++) (b)Hg_(2)^(++) rarr Hg^(++)+Hg (c ) 3AgCl+NO+2H_(2)O rarr 3Ag+3Cl^(-)+NO_(3)^(-)+4H^(+) Given that E_(Fe(+++)//Fe^(++))^(.)=0.77V" "E_(Fe^(++)//Fe)^(.)=-0.44V E_(Hg^(+-)//Hg)^(.)=0.85V" "E_(Hg^(++)//Hg_(2))^(.)=0.92V E_(AgCl//Ag)^(.)=0.22V " "E_(NO_(3)//NO)^(.)=0.96V

What is the standard reduction potential (E^(@)) for Fe^(3+) to Fe ? Given that : Fe^(2+) + 2e^(-) to Fe, E_(Fe^(2+)//Fe)^(@) =-0.47V Fe^(3+) + e^(-) to Fe^(2+), E_(Fe^(3+)//Fe^(2+))^(@) = +0.77V

What is the standard reducing potential (E^(@)) for Fe^(3+)to Fe ? (Given that Fe^(2+)+2e^(-)rightarrowFe, E_(Fe^(2+)//Fe^(@)) =-0.47V Fe^(3+) + e^(-)to Fe^(2+) , E_(Fe^(3+)//Fe^(2+))^(@)= +0.77V

E_(Mn^(3+)//Mn^(2+))^@ is highly positive than that of E_(Cr^(3+)//Cr^(2+))^@orE_(Fe^(3+)//Fe^(2+))^@ because

(i) On the basis of the standard electrode potential values stated for acid solutions, predict whether Ti^(4+) species may be used to oxidise Fe(II) to Fe(III) {:(Ti^(4+) + e^(-) to Ti^(3+), E^(@) = +0.01V), (Fe^(3+) + e^(-) to Fe^(2+), E^(@)= +0.77V):} (ii) Based on the data arrange Fe^(3+), Mn^(2+) " and " Cr^(2+) in the increasing order of stability of +2 oxidation state. (Give a brief reason) E_(Cr^(3+)//Cr^(2+))^(@) = -0.4V E_(Mn^(3+)//Mn^(2+))^(@) = +1.5V E_(Fe^(3+)//Fe^(2+))^(@) = +0.8V

Given : E_(Fe^(3+)//Fe)^(@) = -0.036V, E_(FE^(2+)//Fe)^(@)= -0.439V . The value of electrode potential for the change, Fe_(aq)^(3+) + e^(-)rightarrow Fe^(2+) (aq) will be :

Consider the following E^(@) values E^(@) values E_(Fe^(3+)//Fe^(2+))^(@)= 0.77v , E_(Sn^(2+)//Sn)^(@) = -0.14 under standard condition the potential for the reaction Sn_(s)+ 2Fe^(3+)(aq)rightarrow 2Fe^(2+)(aq) + Sn^(2+) (aq) is :