1. Calculate the Empirical Formula for a compound with the following composition: 46.16% carbon; 53.84% nitrogen 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: CN Next, find the molecular formula if the molecular mass is 52.04 g/mol. Molecular Formula: C2N2C2N2 1

2. Calculate the Empirical Formula for a compound with the following composition: 3.18g carbon; 0.40g hydrogen 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: C2H3C2H3 Next, find the molecular formula if the molecular mass is 135.23 g/mol. Molecular Formula: C 10 H 15 2

3. Calculate the Empirical Formula for a compound with the following composition: 2.458g carbon; 0.459g hydrogen 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: C4H9C4H9 Next, find the molecular formula if the molecular mass is 114.23 g/mol. Molecular Formula: C 8 H 18 3

4. Calculate the Empirical Formula for a compound with the following composition: 40.00% carbon; 6.714% hydrogen; and 53.29% oxygen 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: CH 2 O Next, find the molecular formula if the molecular mass is 180.16 g/mol. Molecular Formula: C 6 H 12 O 6 4

5. Calculate the Empirical Formula for a compound with the following composition: 81.71% carbon; 18.29% hydrogen 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: C3H8C3H8 Next, find the molecular formula if the molecular mass is 132.29 g/mol. Molecular Formula: C 9 H 24 5

6. Calculate the Empirical Formula for a compound with the following composition: 36.37% carbon; 6.104% hydrogen; and 57.53% fluorine 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: CH 2 F Next, find the molecular formula if the molecular mass is 66.05 g/mol. Molecular Formula: C2H4F2C2H4F2 6

7. Calculate the Empirical Formula for a compound with the following composition: 40.80% carbon; 5.136% hydrogen; and 54.06% oxygen 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: C2H3O2C2H3O2 Next, find the molecular formula if the molecular mass is 117.76 g/mol. Molecular Formula: C4H6O4C4H6O4 7

8. Calculate the Empirical Formula for a compound with the following composition: 51.47% carbon; 8.638% hydrogen; and 39.89% nitrogen 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: C3H6N2C3H6N2 Next, find the molecular formula if the molecular mass is 140.02 g/mol. Molecular Formula: C 6 H 12 N 4 8

9. Calculate the Empirical Formula for a compound with the following composition: 3.056g carbon; 0.257g hydrogen; 0.677g oxygen; and 0.595g nitrogen 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: C 6 H 6 NO Next, find the molecular formula if the molecular mass is 324.36 g/mol. Molecular Formula: C 18 H 18 N 3 O 3 9

10. Calculate the Empirical Formula for a compound with the following composition: 49.02% carbon; 2.743% hydrogen; and 48.24% chlorine 1)Change % to grams (if needed) 2)Convert grams to moles 3)Divide by smallest 4)Multiply to get all whole numbers Empirical Formula: C 3 H 2 Cl Next, find the molecular formula if the molecular mass is 220.5 g/mol. Molecular Formula: C 9 H 6 Cl 3 10