Question

4 Fe(s) + 3O2(g) --> 2Fe2O3(g) In Certain reaction, 27.3 g of iron is reacted with 45.8 g of Oxygen. What is the limiting reactant?

Answer 1

Look at the stoichiometry of the reaction....

Explanation:

`underbrace(4Fe(s))_"223.2 g" + underbrace(3O_2(g))_"96.0 g" rarr underbrace(2Fe_2O_3(s))_"319.4 g"`

And so we simply interrogate the molar quantities of metal and oxidant...

`"Moles of iron"=(27.3*g)/(55.8*g*mol^-1)=0.494*mol`

`"Moles of dioxygen"=(45.8*g)/(32.0*g*mol^-1)=1.43*mol`

Clearly, dioxygen is in stoichiometric excess, and thus iron is the limiting reagent .... at MOST, we can make `0.247*mol` ferric oxide. Agreed?