`E^(Theta)` values for the couples `Cr^(3+)//Cr^(2+)` and `Mn^(3+)//Mn^(2+)` -0.41 and +1.51 volts respectively. Considering these values select the correct option from the following statements

E^(Theta) value for the couple Cr^(3+)//Cr^(2+) and Mn^(3+)//Mn^(2+) are -0.41 and +1.51 volts respectively. Considering these value select the correct option from the following statements.

E^(Theta) value for the couple Cr^(3+)//Cr^(2+) and Mn^(3+)//Mn^(2+) are -0.41 and +1.51 volts respectively. Considering these value select the correct option from the following statements.

Between the couple Cr^(3+)//Cr^(2+) and Fe^(3+)//Fe^(2+) whose E value is more positive? Why?

The standard redox potentials for the reactions, MN^(2+) + 2e^(-)to Mn and Mn^(3+) + e^(-) are -1.18V and 1.51V respectively. What is the redox potential for the reaction Mn^(3+)+ 3e^(-) to Mn ?

The standard redox potentials for the reactions, MN^(2+) + 2e^(-)to Mn and Mn^(3+) + e^(-) are -1.18V and 1.51V respectively. What is the redox potential for the reaction Mn^(3+)+ 3e^(-) to Mn ?

Why is the E^(Theta) value for the Mn^(3+)//Mn^(2+) couple much postive than for Cr^(3+)//Cr^(2+) or Fe^(3+)//Fe^(2+) ? Example

(a) why is the E^(Theta) value for the Mn^(3+)//Mn^(2+) couple much more positivethan that for Cr^(3+)//Cr^(2+) or Fe^(3+) // Fe^(2+) ? Explain. (b) What is meant by 'disproportionation' of an oxidation state? Give example.

The E_(M^(3+)|M^(2+))^(0) values for Cr, Mn, Fe and Co are -0.41, +1.57V, + 0.77 and +1.97V respectively. For which one of these metals the change in oxidation sate from +2 to +3 is easiest?