Question

Fe + S --> FeS If we have .14 Mol of Fe and .27 Mol of S. Which is the limiting reactant? How many moles of FeS would be produced if the limiting reactant was used up?

Answer 1

Well, you got 1:1 stoichiometry for....

Explanation:

`underbrace(Fe(s) + S(s))_"55.8 g + 32.06 g"rarr` `FeS(s)`

And of course, we should get a MASS of `87.9*g` with respect to `"iron sulfide"`

And if we got molar quantities of `0.14*mol` with respect to iron, and `0.27*mol` with respect to sulfur, then CLEARLY the sulfur oxidant is in stoichiometric excess.

Also clearly, if the reaction proceeds quantitatively, then we get `0.14*mol` `"iron sulfide"`....and what MASS of iron sulfide does this molar quantity represent....??