Using the balanced equation for the next few questions: 4 Fe(s) + 30 (9) - 2Fe2O3(s) How many moles of Iron (11) Oxide would be produced by complete reaction of 0.15
moles of iron? (Be sure to show your work including the mole ratio you used)

0.075 moles of iron oxide would be produced by complete reaction of 0.15  moles of iron.

Explanation:

The balanced reaction is:

4 Fe + 3 O₂ → 2 Fe₂O₃

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

You can apply the following rule of three: if by stoichiometry 4 moles of Fe produce 2 moles of Fe₂O₃, 0.15 moles of Fe produce how many moles of Fe₂O₃?

moles of Fe₂O₃= 0.075

0.075 moles of iron oxide would be produced by complete reaction of 0.15  moles of iron.

nacl is added to the aqueous of what? ? in order to get a proper answer you have to specify the exact composition of the aqueous solution.