Write the half reaction for the reaction
`2Fe^(+3) + 2I^(-) to 2Fe^(+2) + I_(2)`

Calculate the euilibrium constant for the reaction, 2Fe^(3+) + 3I^(-) hArr 2Fe^(2+) + I_(3)^(-) . The standard reduction potential in acidic conditions are 0.77 V and 0.54 V respectivelu for Fe^(3+)//Fe^(2+) and I_(3)^(-)//I^(-) couples.

Calculate the euilibrium constant for the reaction, 2Fe^(3+) + 3I^(-) hArr 2Fe^(2+) + I_(3)^(-) . The standard reduction potential in acidic conditions are 0.77 V and 0.54 V respectivelu for Fe^(3+)//Fe^(2+) and I_(3)^(-)//I^(-) couples.

Calculate the euilibrium constant for the reaction, 2Fe^(3+) + 3I^(-) hArr 2Fe^(2+) + I_(3)^(-) . The standard reduction potential in acidic conditions are 0.77 V and 0.54 V respectivelu for Fe^(3+)//Fe^(2+) and I_(3)^(-)//I^(-) couples.

Write the half reaction for the following redox reaction. 2Fe^(3+)(aq) + 2l (aq) rarr I_2 (s) + 2Fe^(2+) (aq)

Calculate the value of equilibrium constant for the reaction : 2Fe^(3+)+2I^(-) to 2Fe^(2+)+I_(2) Given that E_(cell)^(@)=0.235" V "

Reduction half reaction for the reaction : Fe^(2+)+MnO_(4)^(-)toFe^(3+)+Mn^(2+) is

Given electrode potentials are , Fe^(3+) + e to Fe^(2+), E^@ = 0.771V " " I_2 + 2e to 2I^(-), E^@ = 0.536 V , E^@ cell for the cell reaction, 2Fe^(3+) + 2I^(-) to 2Fe^(2+) + I_2 is

Calculate the equilibrium constant for the reaction : 2Fe^(3+)+3I^(-)hArr 2Fe^(2+)+I_(3)^(-) . Given: Standard reduction potential in acidic conditions is 0.78 V and 0.54 V, respectively, for Fe^(3+)|Fe^(2+) and I_(3)^(-)|I^(-) couples.