how many moles of o2 are needed to produce 3.91 mol fe2o3
Just follow the steps in this worked example problem of stoichiometry.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the number of moles of O2 needed to produce 3.91 mol Fe2O3, we need to refer to the balanced chemical equation.
The balanced equation for the reaction between Fe2O3 and O2 is:
4 Fe2O3 + 3 O2 → 8 FeO + 6 O3
From this equation, we can see that 4 moles of Fe2O3 react with 3 moles of O2.
Using the ratio from the balanced equation, we can set up a proportion:
4 mol Fe2O3 / 3 mol O2 = 3.91 mol Fe2O3 / x mol O2
Simplifying the proportion:
4/3 = 3.91/x
Now, cross multiply:
4x = 3.91 * 3
4x = 11.73
Divide both sides by 4 to solve for x:
x = 11.73 / 4
x ≈ 2.93 mol O2
Therefore, approximately 2.93 moles of O2 are needed to produce 3.91 mol Fe2O3.