The molecular formula for each of the following compound given the data is
<h3>A. How to determine the molecular formula </h3>
We'll begin by calculating the empirical formula. This can be obtained as follow:
- C = 80%
- H = 20%
- Empirical formula =?
Divide by their molar mass
C = 80 / 12 = 6.67
H = 20 / 1 = 20
Divide by the smallest
C = 6.67 / 6.67 = 1
H = 20 / 6.67 = 3
Thus, the empirical formula of the compound CH₃
Thus, the molecular formula of the compound can be obtained as follow
- Empirical formula = CH₃
- Molar mass of compound = 30 g/mol
- Molecular formula =?
Molecular formula = empirical × n = mass number
[CH₃]n = 30
[12 + (3×1)]n = 30
15n = 30
Divide both side by 15
n = 30 / 15
n = 2
Molecular formula = [CH₃]n
Molecular formula = [CH₃]₂
Molecular formula = C₂H₆
Thus, the molecular formula of the compound is C₂H₆
<h3>B. How to determine the molecular formula </h3>
We'll begin by calculating the empirical formula. This can be obtained as follow:
- C = 92.3%
- H = 7.7%
- Empirical formula =?
Divide by their molar mass
C = 92.3 / 12 = 7.7
H = 7.7 / 1 = 7.7
Divide by the smallest
C = 7.7 / 7.7 = 1
H = 7.7 / 7.7 = 1
Thus, the empirical formula of the compound CH
Thus, the molecular formula of the compound can be obtained as follow
- Empirical formula = CH
- Molar mass of compound = 26 g/mol
- Molecular formula =?
Molecular formula = empirical × n = mass number
[CH]n = 26
[12 + 1]n = 26
13n = 26
Divide both side by 13
n = 26 / 13
n = 2
Molecular formula = [CH]n
Molecular formula = [CH]₂
Molecular formula = C₂H₂
Thus, the molecular formula of the compound is C₂H₂
<h3>C. How to determine the molecular formula </h3>
We'll begin by calculating the empirical formula. This can be obtained as follow:
- C = 37.5%
- H = 6.3%
- Cl = 55.8%
- Empirical formula =?
Divide by their molar mass
C = 37.5 / 12 = 3.125
H = 6.3 / 1 = 6.3
Cl = 55.8 / 35.5 = 1.572
Divide by the smallest
C = 3.125 / 1.572 = 2
H = 6.3 / 1.572 = 4
Cl = 1.572 / 1.572 = 1
Thus, the empirical formula of the compound C₂H₄Cl
Thus, the molecular formula of the compound can be obtained as follow
- Empirical formula = C₂H₄Cl
- Molar mass of compound = 127 g/mol
- Molecular formula =?
Molecular formula = empirical × n = mass number
[C₂H₄Cl]n = 127
[(2×12) + (4×1) + 35.5]n = 127
63.5n = 127
Divide both side by 63.5
n = 127 / 63.5
n = 2
Molecular formula = [C₂H₄Cl]n
Molecular formula = [C₂H₄Cl]₂
Molecular formula = C₄H₈Cl₂
Thus, the molecular formula of the compound is C₄H₈Cl₂
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