The equation for reducing iron (iii) oxide with heated carbon is: $\ce{Fe2O3 (s) + 3C (s) + 3CO (g)}$ The mass of carbon needed to produce $100~\mathrm{g}$ iron is?

I honestly do not understand how to do this. Please give me a detailed solution and dumb it down as much as possible.

  • 2
    $\begingroup$ Welcome to Chemistry.SE. Please show us what you have tried to accomplish and have a look at our homework policy. You can also improve formatting by following the guidelines in the help center. For a first start you might want to look at this wikipedia article about blast furnace $\endgroup$ – Martin - マーチン May 22 '14 at 11:53
  • $\begingroup$ @Martin thanks I actually managed to work it out $\endgroup$ – user5583 May 22 '14 at 13:29
  • 4
    $\begingroup$ Would you be kind enough to share your knowledge and post an answer to your question? It might help some other people later on. Thank you very much. $\endgroup$ – Martin - マーチン May 23 '14 at 1:46

It's easy to calculate the mass of carbon. At first you have to write down the chemical equation:

$2~Fe_2O_3 + 3~C \rightarrow 4~Fe + 3 CO_2$

Now you can solve the following equation:

$\frac{m_{C}}{m_{Fe}}=\frac{n_{C} \cdot M_{C}}{n_{Fe} \cdot M_{Fe}}$

$m_{C}=\frac{n_{C} \cdot M_{C} \cdot m_{Fe}}{n_{Fe} \cdot M_{Fe}}$

$m_{C}=\frac{3~mol \cdot 12~\frac{g}{mol} \cdot 100~g}{4~mol \cdot 56~\frac{g}{mol}}$

$m_{C} = 16~g$

You need 16g Carbon to produce 100g Iron.


Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.