Question

Give the equations for the redox reactions taking place in the extraction of iron from
haematite.
In each case state which substance is oxidised and which is reduced.

Answer 1

3Fe +4H20--------->Fe3O4 +4H2
here u see in reactant side the charge on Fe is 0 while on product side the charge on Fe is nearly +2.6 u see here Fe got oxidised and Oxygen get reduced by doing the same process as we done for Fe

Answer 2

to calculate charge i m doing one xample how to do like for Fe
Fe------------> Fe3O4
now here Fe is neutral means no charge o we say FE contain 0 charge
now in Fe3O4 u take the unknown charge be x and use formula:
no of surrounding atom x charge of element to be found + no. of ligand surrounding atom x the charge of ligand=net charge on a molecule
3x + 4(-2)=0
x=+2.6
as we know oxygen contain -2 charge with it :) so for 1 oxygen -2 therfore for 4 oxygen it contain -8 charge by uing formula u get for one FE u had +2.6 charge there for for 3 Fe u ll get +8 charge sso the molecule become neutral

Answer 3

the extraction of iron from haematite.
Fe3O4 +4H2->3Fe +4H20
is n't what the equation should be???

Answer 4

ye right srry @ssh1995 mos is right just reverse thereaction and the proces i told u to calculate charge dodt u ll get which is oxzidised and which is redced :) and thnx mos for correcting me :)