Step 1: Carbon is burned in a limited supply of oxygen to form carbon monoxide. Step 2: The carbon monoxide formed in Step 1 is used to reduce iron(III) oxide to metallic iron and carbon dioxide.

Question

Calculate the mass (in kg) of O2 needed to produce 100 kg of Fe.

Can someone please help me with this and could you please write the equation out for me. Thanks to anyone who helps

Answer 1

Nuts to you three guys. Your answer(s) has/have nothing to do with the post by Jack. I would delete those three posts if I could. Here is the solution to Jack's problem.
2C + O2 ==> 2CO
Fe2O3 + 3CO ==> 2Fe(s) + 3CO2

So 1 mol O2 in eqn 1 = 2 mols CO
In eqn two, 2 mol Fe = 3 mols CO
Multiply eqn 1 by 3 and eqn 2 by 2 to obtain
eqn 1 x 3 is 3 mols O2 = 6 mols CO and
eqn 2 x 2 is 4 mols Fe = 6 mols CO; therefore,
3 mols O2 = 4 mols Fe.

Now, you want 100 kg Fe which is 100,000/55.85 = 1790 mols.
That will require 1790 mols Fe x (3 mols O2/4 mols Fe) = 1790 x 3/4 = ?
Convert that to grams by multiplying by molar mass of O2 (that's 32) = ?
Then convert grams to kg and you have it. Post your work if you have any trouble. As for the three funny guys (hahaha), just forget them.

Answer 2

Thank you DrBob. I got the answer correct and I understand it now.

Answer 3

I would like to apologize as I now know the first 3 gentlemen were correct. I offer my most sincere apologies for any potential damage caused.