1 mole of equimolar mixture of ferric oxalate and ferrous oxalate will require xmole of KMnO4 in acidic medium for complete oxidation, x isis:

a) 0.5 mole b) 0.9 mole c) 1.2 mole d) 4.5 mole

O.9

So you have 1/2 mol Fe2(C2O4)3 and 1/2 mol FeC2O4.

Write the reaction for the ferric salt in which just the C2O4 is oxidized to CO2.
Then write the reactiion for the ferrous salt in which ferrous is oxidized to ferric and the oxalate is oxidized to CO2. Then add the mols together from the two equations.

To determine the amount of KMnO4 required for the complete oxidation of a mole of the equimolar mixture of ferric oxalate and ferrous oxalate, we need to balance the redox equation and calculate the stoichiometric coefficients.

The balanced equation for the reaction between KMnO4 and oxalates in acidic medium can be written as follows:

5C2O4^2- + 2MnO4^- + 16H^+ → 10CO2 + 2Mn^2+ + 8H2O

From the balanced equation, we can see that for every 2 moles of KMnO4, we need 5 moles of C2O4^2- ions. Since the equimolar mixture of ferric and ferrous oxalate contains 1 mole of each, the total moles of C2O4^2- ions in the mixture is 2 moles.

So, for the complete oxidation of a mole of the equimolar mixture, we would need 2/5 moles of KMnO4.

Now let's calculate x:

x = 2/5 = 0.4 moles

Therefore, the answer is not listed among the options provided.

Yes