Question

Read the chemical equation.

Answer 1

Answer:- D. 1.8 moles of Fe and $2.7molCO_2$ .

Solution:- The balanced equation is:

$Fe_2O_3+3CO\rightarrow 2Fe+3CO_2$

let's first figure out the limiting reactant using the given moles and mol ratio:

$1.8molFe_2O_3(\frac{3molCO}{1molFe_2O_3})$

= 5.4 mol CO

From calculations, 5.4 moles of CO are required to react completely with 1.8 moles of Iron(III)oxide but only 2.7 moles of CO are available. It means CO is limiting reactant.

Products moles depends on limiting reactant. Let's calculate the moles of each reactant formed for given 2.7 moles of CO.

$2.7molCO(\frac{2molFe}{3molCO})$

= 1.8 mol Fe

$2.7molCO(\frac{3molCO_2}{3molCO})$

= $2.7molCO_2$

So, the correct choice is D.  1.8 moles of Fe and $2.7molCO_2$ are formed.