Questions regarding mass/mole used

Question

2Fe2O3(s) 3C(s) heat <--> 4Fe(s) 3CO2(g)

a) 229 grams of Iron Oxide is added.

i) Number of moles of Iron Oxide reacted?

229/[4(55.847) 6(16)] = 0.717 mol

ii) Number of mole of Carbon consumed?

iii) Mass of carbon required?

Is question a(i) correct?

And I'm having trouble figuring out (ii) and (iii).

Any help to any question is appreciated!

Thanks in advanced.

Answer 1

i)Since they only give you the mass of one the reactants we can assume that the other reactant is in excess. So iron(III)oxide is the limiting reagent. To find out how much iron(III) oxide reacts just divide the mass of the mineral by its molar mass.

229g *(mol/160g) = 1.43moles of Fe2O3(s)

ii) To find out the moles of carbon produced you muliply the number of moles of iron mineral by the mole ratio. Which is 3C : 2 Fe2O3

1.43moles of Fe2O3(s) *(3 moles C/2 moles of Fe2O3) = 2.15 moles C

iii) To find the mass of carbon simply multipy the moles of C by the molar mass of C.

2.15 moles C (12g/mol) = 25.8g of C