Question

Iron is produced from its ore by the reactions. How many moles of O2(g) are needed to produce 4.6 moles of Fe(s)?

a. 2.3 moles
b. 3.0 moles
c. 4.6 moles
d. 6.9 moles

Answer 1

To produce 4.6 moles of Fe(s), 3.0 moles of O2(g) are needed, according to the balanced chemical equation.

Step-by-step explanation:

To determine the number of moles of O2(g) needed to produce 4.6 moles of Fe(s), we need to use the balanced chemical equation for the reaction. The balanced equation is:

4Fe2O3(s) + 3O2(g) → 8Fe(s)

From the equation, we can see that 3 moles of O2 are needed to produce 8 moles of Fe. Therefore, we can set up a proportion to find the number of moles of O2 needed:

3 moles O2 / 8 moles Fe = x moles O2 / 4.6 moles Fe

Cross-multiplying and solving for x, we find that x = 4.6 × (3 moles O2 / 8 moles Fe) = 1.725 moles O2.

Therefore, the correct answer is 1.725 moles, which is closest to option b. 3.0 moles.