Question

What mass of CO is needed to react completely with 55.0 g of Fe2O3 in the reaction: Fe2O3(s) + CO(g) → Fe(s) + CO2(g)?
4.82 g CO
9.64 g CO
14.5 g CO
28.9 g CO

Answer 1

Answer:- 28.9 grams of CO are needed to react with 55.0 grams of Iron(II)oxide.

Solution:- The balanced equation for the given reaction is:

$Fe_2O_3(s)+3CO(g)\rightarrow 2Fe(s)+3CO_2$

From this equation, 1 mol of Iron(II)oxide reacts with 2 moles of carbon monoxide. First of all we convert given grams of Iron(II)oxide to moles and multiply by the mol ratio to get the moles of CO. Further the moles of CO are multiplied by it's molar mass to find out it's grams.

Molar mass of $Fe_2O_3$ is 159.69 gram per mol and the molar mass of CO is 28 gram per mol. The calculations are shown below:

$55.0gFe_2O_3(\frac{1molFe_2O_3}{159.69gFe_2O_3})(\frac{3molCO}{1molFe_2O_3})(\frac{28gCO}{1molCO})$

= 28.9 g CO

So, 28.9 grams of CO are needed to react completely with 55.0 grams of Iron(II)oxide.