Question

A 2.00g sample of Fe3O4 is reacted with with 8.00g of O2 to produce Fe2O3.
a) What mass of Fe2O3 will be produced?
b) What mass of Fe2O3 will actually be produced if the percentage yield for reaction is 85% produced?

Answer 1

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Answer 2

\(\sf 4 Fe_3O_4 + O_2 = 6 Fe_2O_3\)
This will be the balanced equation. Now 4 moles of Fe3O4 reacts with 1 mole of O2 to form 6 moles of Fe2O3

Answer 3

How do I use the information given to work out the two problems given?