Question

7) Using the following balanced equation 4 Fe(s) + 302(g) → 2Fe2O3(s)

a) How many moles of product 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

Step-by-step explanation:

Looking at the balanced equation, 4 moles of Fe(s) react with 3 moles of
`O_(2)` to produce 2 moles of
`Fe_(2)O_(3)` (s). In other words, for every 4 moles of Fe(s) used, there are 2 moles of product. The mole ratio is therefore 4:2, or 2:1. In other words, you divide the moles of Fe by two to find the moles of product.

There are 0.15 moles of Fe, so the moles of product should be half of this according to the molar ratio.

• 0.15 / 2 = 0.075

Your answer is 0.075 moles.

Hope this helps!