Given the reaction:
4Fe(s)+3O2(g)→2Fe2O3 ΔH= -1652 kJ
a) How much heat is released when 4.00 mol iron is reacted with excess O2?
b) How much heat is released when 1.00 mol Fe2O3 is produced?
c) How much heat is released when 1.00g iron is reacted with excess O2?
d) How much heat is released when 10.0g Fe and 2.00g O2 are reacted?
I have an idea of how to do this, but i am really not sure I having a feeling it's pretty simple, but can anyone please explain it me?
a) 4.00 mol iron ----1652 kJ
b)1.00 mol Fe2O3 -----1652 kJ / 2
c) 1.00g iron ------1652 KJ / molar mass of Fe
d )10.0g Fe and 2.00g O2
here limiting reactant is O2
----1652 kJ X moles of O2 in 2 g / 3 moles of O 2