Write a balanced equation for the oxidation of Iron from the 2+ oxidation state to the 3+ oxidation state using the manganate ion.

Firstly, we need to write a balanced equation for the oxidation of Fe2+ to Fe3+ . We know that when something is oxidised, it is losing electrons, making the half equation: Fe2+ ---> Fe3+ + e- (we can check this by ensuring the charges on each side of the equation are equal). If iron is being oxidised, the manganate ion must be being reduced and so we write a half equation for the reduction of Mn(VII) to Mn(II): MnO4- --->   Mn2+. We must now balance the equation, first for number of atoms of each element by adding water and hydrogen ions: MnO4- + 8H+ --->   Mn2+ + 4H2O. We then balance for charge by adding electrons: MnO4- + 8H+ + 5e- --->   Mn2+ + 4H2O. Finally, we must combine the two half equations by multiplying everything in the equation for oxidation of iron by 5 so that, once combined, the number of electrons on each side of the equation cancel each other out. This leave us with the final equation: 5Fe2+ + MnO4- + 8H+ --->  5Fe3+ + Mn2+ + 4H2O.

Answered by Paige M. Chemistry tutor

11050 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

The following equilibrium is set up in a glass syringe. 2(NO2) (brown gas) ‹-› N2O4 (colourless gas) ∆H = -58 kJmol-1. Using le Chatelier's principle, predict and explain how heating up the mixture would affect it's appearance.


Why do the atomic radii of the elements decrease across a period?


Explain why the enthalpy of lattice dissociation of potassium oxide is less endothermic than that of sodium oxide.


Describe the shape of and bonding in a molecule of benzine. Explain why benzene doesn't readily undergo reactions.


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2024

Terms & Conditions|Privacy Policy
Cookie Preferences