Question

Using the following balanced equation 4 Fe(s) + 3O2(g) -> 2Fe2O3(s)

b) How many moles of product would be produced by complete reaction of 0.15 moles of oxygen gas? (Be sure to
show your work including the mole ratio you used)

Answer 1

0.225 moles

Step-by-step explanation:

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

There are 0.15 moles of
`O_(2)`, so the moles of product should be 3/2 of this according to the molar ratio.

0.15 *
`(3)/(2)` = 0.225

Your answer is 0.225 moles.

Hope this helps!