posted by claire .
Iron and oxide react to form iron(lll) oxide: 4Fe(s) + 3O2(g)+ 2FeO2(s) Determine the limiting reactant in each of the following mixtures of reactants: 2.0 moles of Fe and 6.0 moles of O2
Here is a link for solving stoichiometry problems. http://www.jiskha.com/science/chemistry/stoichiometry.html
First use 2.0 moles Fe and ignore oxygen. Second, use 6.0 moles oxygen and ignore Fe. Calculate, in each case, moles of the product. You get different answers; of course, only one can be right. In limiting reagent problems, the smaller value of the product is ALWAYS the correct one to choose and the reagent producing that vale is the limiting reagent.