2. Actual Yield The amount of product formed from the actual chemical reaction and it is usually less than the theoretical yield.

3. Theoretical Yield The maximum amount of product which could be produced by the complete reaction of the limiting reactant.

5. Sample Problem: What is the % yield of H 2 O if 138 g H 2 O is produced from 16 g H 2 and excess O 2 ?

6. What is the % yield of H 2 O if 58 g H 2 O are produced by combining 60 g O 2 and 7.0 g H 2 ?

7. Molecular formula specifies both the relative and the actual number of atoms in a molecule.

8. Empirical formula specifies the smallest whole-number ratio of atoms of the element of a compound.

9. Molecular Formula NamesEmpirical Formula C2H6C2H6 EthaneCH 3 H2O2H2O2 Hydrogen Peroxide HO H2C2O4H2C2O4 Oxalic Acid HCO 2

10. What is the empirical formula of a compound containing 70.19 % Lead, 8. 14% Carbon and 21.67 % Oxygen.

11. Step 1: Assume that the sample is 100 g so that the given percentage of each element is the mass in grams of the element.

12. Step 2: Calculate the number of moles of each element.

13. Step 2: Calculate the number of moles of each element.

14. Step 3: Get the ratio of the elements by dividing the calculated moles by the smallest quantity.

15. Find the empirical formula of the oxide formed when 1.06 g of aluminium burns completely in oxygen, producing 2.06 g of oxide?

16. If the empirical formula of the compound is CH 2 O and its molecular mass is 181 g, What is the molecular formula?

17. Step 1: Get the Empirical Formula Mass

18. Step 2: Get the the value of n,the multiplier of the subscripts of the empirical formula.

19. Step : Multiply the value of n to the subscripts of the empirical formula.

20. What is the molecular formula of a substance containing 43.64% phosphorus and 56.36% oxygen by mass? Its molecular mass is 141.9 g.