Question

Consider the following balanced chemical equation:

4Fe(s) + 3O₂(g) → 2Fe₂O₃(s)

a. How many moles of iron are required to react with 15.7 moles of O₂?

moles Fe

b. How many moles of O₂ are required to react with 15.7 moles of iron?

moles O₂

c. How many moles of O₂ are required to form 15.7 moles of Fe₂O₃? Assume excess Fe.

moles O₂

d. How many molecules of O₂ are required to form 15.7 moles of Fe₂O₃? Assume excess Fe.

× 10^{(Click to select)2122232425} molecules O₂

Answer 1

The balanced chemical equation:

      4Fe(s) + 3O2(g)   ---> 2Fe2o3(s)

from the balanced equation,

a. 3 moles of O2 reacts with 4 moles of Fe

therefore, 15.7 moles of O2 reacts with 4*15.7/3= 20.93 moles of Fe

b. 4 moles of Fe reacts with 3 moles of O2

therefore, 15.7 moles of Fe reacts with 3*15.7/4 = 11.775 moles of O2

c. 2 moles of Fe2O3 is produced by 3 moles of O2

therefore, 15.7 moles of Fe2O3 is produced from 3*15.7/2 = 23.55 moles of O2

d. 15.7 moles of Fe2O3 is produced from 23.55 moles of O2

therefore,the number of molecules of O2 are required to form 15.7 moles of Fe2O3 is 23.55*6.023*10^23 = 1.418*10^25 molecules