How many moles of Fe3O4 are required to supply enough iron to prepare 0.752 mol Fe2O3?
Follow the template for the UF6 problem.
To determine how many moles of Fe3O4 are required to supply enough iron to prepare 0.752 mol Fe2O3, it's important to understand the balanced chemical equation for the reaction between Fe3O4 and Fe2O3.
The balanced chemical equation is:
Fe3O4 + 2Fe2O3 -> 6FeO
This equation tells us that for every 1 mole of Fe3O4, we can produce 2 moles of Fe2O3.
Now, we can set up a ratio using the stoichiometric coefficients from the balanced equation to determine the number of moles of Fe3O4 needed.
1 mole of Fe3O4 produces 2 moles of Fe2O3
Therefore,
1 mole of Fe2O3 requires (1/2) moles of Fe3O4
To find the number of moles of Fe3O4 needed to produce 0.752 mol Fe2O3, we can multiply the given amount by the ratio calculated above:
Number of moles of Fe3O4 = 0.752 mol Fe2O3 × (1/2) mol Fe3O4/1 mol Fe2O3
= 0.376 mol Fe3O4
Therefore, 0.376 moles of Fe3O4 are required to supply enough iron to prepare 0.752 mol Fe2O3.