[Chemistry] Chemical Reaction, limiting reactants and result stoichiometry

1. Nov 13, 2012

bnosam

1. The problem statement, all variables and given/known data

609.5 grams of vanadium (II) oxide, VO, and 832 grams of iron(III) oxide, Fe2O3, react according to the equation, which substance(s) and how many grams of each would be in the tube after the reaction completes? 3 points

2. Relevant equations
Equation:

2 VO + 3 Fe2O3 -> 6 FeO + V2O5

3.

1 mol VO = 66.94 g
1 mol Fe2O3 = 159.70 g

$\frac{609.5 g VO}{66.94 g/mol VO} = 9.11 mol VO$

$\frac{832 Fe_{2}O_{3}}{159.7 g/mol Fe_{2}O_{3}} = 5.21 molFe_{2}O_{3}$

3. The attempt at a solution
$\frac{9.11 mol VO * 3 mol Fe_{2}O_{3}}{2 mol VO} = 13.6 mol Fe_{2}O_{3}$

$\frac{5.21 mol Fe_{2}O_{3} * 2 mol VO}{3 mol Fe_{2}O_{3}} = 3.47 mol VO$

So the limiting reactant would be $Fe_{2}O_{3}$, right?

I'm not quite sure where to go after this, any pointers in the right direction?

Thanks :)

2. Nov 13, 2012

AGNuke

Consume all the Limiting reagent to form products. Find the amount of excess reagent used with LR, find the amount of products. Balanced Stoichiometric equation helps.