Consider the cell potentials `E_(Mg^(2+)|Mg)^(0)=-2.37V` and `E_(Fe^(3+)|Fe)^(0)=-0.04V`
The best reducing agent would be

Consider the celll ptentiasl E_(Mf^(2+//Mg)^@ =- 2.37 V and E_(Fe^(3+)//Fe)^@ =- 0.04 V . The best reducing agnet would be .

Will Mg reduce CuSO_4 ? E_(Mg,Mg^(2+))^@=+2.36V and E_(Cu,Cu^(2+))^@=0.34V

E_(Mg//Mg^(2+))^(@)=2.37V E_(Al^(3+)//Al)^(@)=1.66V E_("cell")^(@) and the cell reaction is

Consider the following E^(0) values E_(Fe^(3+) // Fe^(2+))^(0) = + 0.77 V , E_(Sn^(2+) // Sn)^(0)=-0.14 V Under standard condition the potential for the reaction Sn_((s)) + 2Fe_((aq))^(3+) to 2Fe_((aq))^(2+) + Sn_((aq))^(2+) is

If E_(Fe^(2+)//Fe)^(@)=-0.440 V and E_(Fe^(3+)//Fe^(2+))^(@)=0.770 V , then E_(Fe^(3+)//Fe)^(@) is -

Given that E_(Fe^(3+)|Fe)^(0) and E_(Fe^(2+)|Fe)^(0) are -36V and -0.439V , respectively . The value of E_(Fe^(3+),Fe^(2+)|Pt)^(0) would be

Calculate E_("cell")^(@) of the cell Mg|Mg^(2+)||Cu^(+)|Cu Given : E_(Mg^(2+)|Mg)^(@)=-2.37V and E_(Cu^(+)|Cu)^(@)=+0.15V .