Transcript Empirical-Molecular_Practice

1
Calculate the Empirical Formula for a
compound with the following composition:
46.16% carbon; 53.84% nitrogen
1)
2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
CN
Next, find the molecular formula if the
molecular mass is 52.04 g/mol.
Empirical Formula:
Molecular Formula:
C2N2
2
Calculate the Empirical Formula for a
compound with the following composition:
3.18g carbon; 0.40g hydrogen
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2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
C2H3
Next, find the molecular formula if the
molecular mass is 135.23 g/mol.
Empirical Formula:
Molecular Formula:
C10H15
3
Calculate the Empirical Formula for a
compound with the following composition:
2.458g carbon; 0.459g hydrogen
1)
2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
C4H9
Next, find the molecular formula if the
molecular mass is 114.23 g/mol.
Empirical Formula:
Molecular Formula:
C8H18
4
Calculate the Empirical Formula for a
compound with the following composition:
40.00% carbon; 6.714% hydrogen; and 53.29% oxygen
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2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
CH2O
Next, find the molecular formula if the
molecular mass is 180.16 g/mol.
Empirical Formula:
Molecular Formula:
C6H12O6
5
Calculate the Empirical Formula for a
compound with the following composition:
81.71% carbon; 18.29% hydrogen
1)
2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
C3H8
Next, find the molecular formula if the
molecular mass is 132.29 g/mol.
Empirical Formula:
Molecular Formula:
C9H24
6
Calculate the Empirical Formula for a
compound with the following composition:
36.37% carbon; 6.104% hydrogen; and 57.53% fluorine
1)
2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
CH2F
Next, find the molecular formula if the
molecular mass is 66.05 g/mol.
Empirical Formula:
Molecular Formula:
C2H4F2
7
Calculate the Empirical Formula for a
compound with the following composition:
40.80% carbon; 5.136% hydrogen; and 54.06% oxygen
1)
2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
C2H3O2
Next, find the molecular formula if the
molecular mass is 117.76 g/mol.
Empirical Formula:
Molecular Formula:
C4H6O4
8
Calculate the Empirical Formula for a
compound with the following composition:
51.47% carbon; 8.638% hydrogen; and 39.89% nitrogen
1)
2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
C3H6N2
Next, find the molecular formula if the
molecular mass is 140.02 g/mol.
Empirical Formula:
Molecular Formula:
C6H12N4
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)
2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
C6H6NO
Next, find the molecular formula if the
molecular mass is 324.36 g/mol.
Empirical Formula:
Molecular Formula:
C18H18N3O3
10
Calculate the Empirical Formula for a
compound with the following composition:
49.02% carbon; 2.743% hydrogen; and 48.24% chlorine
1)
2)
3)
4)
Change % to grams (if needed)
Convert grams to moles
Divide by smallest
Multiply to get all whole numbers
C3H2Cl
Next, find the molecular formula if the
molecular mass is 220.5 g/mol.
Empirical Formula:
Molecular Formula:
C9H6Cl3