Question

Why CO and H2 can reduce hot iron(III) oxide to iron?
For CO, is it because it can undergo redox reaction with the equation
6CO +2Fe2O3 -> 6CO2 + 4Fe ?

Answer 1

H2 will oxidize to water.

CO will oxidize to CO2.

Answer 2

Why would H2 oxidized to H2O in this case?

Answer 3

Fe2O3 + 3 H2 -->2 Fe + 3 H2O

Answer 4

this is how (but i think you are looking for why...)

Answer 5

Hmm... I know that equation... but why can it happen? :S

Answer 6

It depends on the Gibbs free energy change linked to the reactions ΔG(T).
See : http://en.wikipedia.org/wiki/Ellingham_diagram

Answer 7

H2 cannot reduce Iron oxide. it is down the reactivity series (below iron) which means the reduction cannot take place.

Answer 8

Sorry, but that doesn't make sense.... Fe(III) ion ranks lower in ECS than H2...

Answer 9

http://www.zephyrus.co.uk/thereactivityseries.html

Answer 10

Sorry, a little messy with my book :S

Answer 11

It Does make sense. We are not talking aqueous solutions here and reactivity series, but reactions between solids and gases at different temperatures.
Elligham's diagram for CO2/CO and H2O/H2 is as follows:

It shows that above 1100K, H2 is a stronger reducing agent than CO.

Diagram for iron and hydrogen is:
1. Whatever the temperature, H2 will reduce Fe2O3 to Fe3O4
2. Above the temperature of the circled point (I do not have its value, it is slightly below 950K), H2 will even reduce Fe3O4 to Fe.