The true molecular formula of the compound is C₂ClF₅
<h3>Determination of the mole of the compound </h3>
- Volume (V) = 428 cm³ = 428 / 1000 = 0.428 L
- Pressure (P) = 99.06 KPa = 99.06 / 101.325 = 0.978 atm
- Temperature (T) = 24.3˚C = 24.3 + 273 = 297.3 K
- Gas constant (R) = 0.0821 atm.L/Kmol
- Number of mole (n) =?
The number of mole can be obtained as by using the ideal gas equation as illustrated below:
n = PV / RT
n = (0.978 × 0.428) / (0.0821 × 297.3)
n = 0.017 mole
<h3>How to determine the molar mass </h3>
- Mole = 0.017 mole
- Mass = 2.650 g
- Molar mass =?
Molar mass = mass / mole
Molar mass = 2.650 / 0.017
Molar mass = 155.88 g/mol
<h3>How to determine the empirical formula</h3>
- Carbon (C) = 15.5%
- Chlorine (Cl) = 23%
- Fluorine (F) = 61.5%
- Empirical formula =?
Divide by their molar mass
C = 15.5 / 12 = 1.292
Cl = 23 / 35.5 = 0.648
F = 61.5 / 19 = 3.237
Divide by the smallest
C = 1.292 / 0.648 = 2
Cl = 0.648 / 0.648 = 1
F = 3.237 / 0.648 = 5
Thus, the empirical formula of the compound is C₂ClF₅
<h3>How to determine the molecular formula </h3>
- Molar mass of compound = 155.88 g/mol
- Empirical formula = C₂ClF₅
- Molecular formula =?
Molecular formula = empirical × n = molar mass
[C₂ClF₅]ₙ = 118.084
[(12×2) + 35.5 + (19×5)]ₙ = 155.88
154.5n = 155.88
Divide both side by 154.5
n = 155.88 / 154.5
n = 1
Molecular formula = [C₂ClF₅]ₙ
Molecular formula = [C₂ClF₅]1
Molecular formula = C₂ClF₅
Learn more about empirical and molecular formula:
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