Question

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)

Answer 1

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

Step-by-step 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:

• Fe: 4 moles
• O₂: 3 moles
• Fe₂O₃: 2 moles

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 Fe_(2) O_(3) =(0.15 moles of Fe*2 moles of Fe_(2) O_(3) )/(4 moles of Fe)`

moles of Fe₂O₃= 0.075

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