6. If 8.00 moles H2 are to be reacted, how many moles of O2 are needed for stoic

Question

6. If 8.00 moles H2 are to be reacted, how many moles of O2 are needed for stoichiometric equivalence? Consider the following reaction for questions 7-8 4Fe+3O2 2Fe:03 7. To form four particles of FeO a. How many atoms of Fe are needed? b. How many molecules of O; are needed? 8. If 20 atoms of Fe are mixed with 20 molecules of oxygen and the reaction goes to completion a. The Fe consumes how much O as it reacts? b. How much O is left over? c. How many particles of Fe:O are formed? d. Which reactant is in excess? e. Which reactant is limiting?

Explanation / Answer

7. Reaction is 4 Fe + 3 O2 ==== 2 Fe2O3

4 atoms of Fe are required to form 2 particles of Fe2O3 , we want 4 particles of Fe2O3, 4 is the double of 2 so we need the double amount of Fe

4 * 2 = 8 atoms of Fe are required

The same goes for the Oxygen O2

3 * 2 = 6 moles of O2 are required

8. There are 20 atoms of Fe and 20 molecules of O2

4 atoms of Fe require 3 molecules of O2 so, lets double this number

8 atoms of Fe require 6 molecules of O2,

lets multiply by 5 the original relationship

20 atoms of Fe require 15 molecules of O2

15 molecules of O2 will be consumed

Originally there are 20 molecules of O2 so

20 - 15 = 5 molecules of O2 will be left

lets go back to the original relationship for part C

4 atoms of Fe will produce 2 molecules of Fe2O3

20/4 = 5

multiply by 5 the relationship to get

20 atoms of Fe will producte 10 molecules of Fe2O3 so

10 molecules of Fe2O3 will be produced

Since all the Fe will be consumed and some O2 will remain then

O2 is in excess

Fe is the limiting reactant

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