Given #200*g# masses each of sodium metal, and ferric oxide.....can you address..?

...which reagent is in excess in the context of iron reduction....?

#Fe_2O_3(s) + 6Na(s) rarr 3Na_2O(s) + 2Fe(s)#

1 Answer
anor277
Mar 25, 2017

You have the stoichiometric equation:..........

Explanation:

#6Na + Fe_2O_3 rarr 3Na_2O + 2Fe#.

#"Moles of natrium"# #=# #(200*g)/(22.99*g*mol^-1)=8.70*mol#

#"Moles of ferric oxide"# #=# #(200*g)/(159,69*g*mol^-1)=1.25*mol#

Given the #6:1# stoichiometry, the natrium is in excess, and all the ferric oxide should be reduced to the metal.

Note that this would be an extremely expensive and impractical way of producing iron metal. Far better (and miles cheaper) to produce iron the traditional way, and heat it up with coke (i.e. carbon), and reduce the iron while producing #CO# and #CO_2#:

#Fe_2O_3 + 3C rarr 2Fe + 3COuarr#

Are these redox equations?

Related questions
See all questions in Stoichiometry
Impact of this question
1196 views around the world
You can reuse this answer
Creative Commons License