Dilute HCI oxidises metallic Fe to `Fe^(2+)`.

If equal volumes of 0.1 M KMnO_(4) and 0.1 M K_(2)Cr_(2)O_(7) solutions are allowed to oxidise Fe^(2+) to Fe^(3+) in acidic medium, then Fe^(2+) oxidised will be:

Equal volumes of 1M KMnO_4 and 1M K_2Cr_2O_7 solution are allowed to oxidise Fe^(2+) ions to Fe^(3+) ions in acidic medium. The number of moles of Fe^(2+) ions oxidised in the two cases are in the ratio:

Given the standard oxidation potentials Fe overset(+0.4V)rarr Fe^(2+) (aq.) overset(-0.8V)rarr Fe^(3+) (aq.) Fe overset(+0.9V)rarr Fe(OH)_(2) overset(0.6V)rarr Fe(OH)_(3) It is easier to oxidise Fe^(2+) " to " Fe^(3+)in

Calculate the magnetic moments of Fe^(2+) and Fe^(3+)

If equal volumes of 1 M KMnO_(4) and 1M K_(2)Cr_(2)O_(7) solutions are allowed to oxidise Fe(II) to Fe(III) in acidic medium, then Fe(II) oxidised will be

The number of moles of KMnO_(4) required to oxidise 1 mol of Fe(C_(2)O_(4)) in acidic medium is

(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

Fe^(3+) compounds are more stable than Fe^(2+) compounds because

Find the oxidation number of Fe in [Fe(H_2O)_6]^(3+)

Assertion (A) : Fe^(3+) (g) ion is more stable than Fe^(2+)(g) ion. Reason (R) : Fe^(3+) ion has more number of unpaired electrons than Fe^(2+) ion.