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Sagot :
A. The molecular mass of the compound is 77.9 g/mol
B. The molecular formula of the compound is C₆H₆
Determination of the mole of the compound
We'll begin by calculating the number of mole of compound using the ideal gas equation as shown below:
- Volume (V) = 102 cm³ = 102 / 1000 = 0.102 L
- Temperature (T) = 373 K
- Pressure (P) = 775 mmHg = 775 / 760 = 1.02 atm
- Gas constant (R) = 0.0821 atm.L/Kmol
- Number of mole (n) =?
n = PV / RT
n = (1.02 × 0.102) / (0.0821 × 373)
n = 0.0034 mole
A. Determination of the molecular mass of the compound.
- Mass = 0.265 g
- Number of mole = 0.0034 mole
- Molecular mass =?
Molecular mass = mass / mole
Molecular mass = 0.265 / 0.0034
Molecular mass of compound = 77.9 g/mol
B. Determination of the molecular formula of the compound.
We'll begin by calculating the empirical formula of the compound.
- Carbon (C) = 92.24%
- Hydrogen (H) = 7.76%
Empirical formula =?
Divide by their molar mass
C = 92.24 / 12 = 7.69
H = 7.76 / 1 = 7.76
Divide by the smallest
C = 7.69 / 7.69 = 1
H = 7.76 / 7.69 = 1
Thus the empirical formula of the compound is CH
Finally, we shall determine the molecular formula.
- Molecular mass = 77.9 g/mol
- Empirical formula = CH
- Molecular formula =?
Molecular formula = empirical × n = molecular mass
[CH]n = 77.9
[12 + 1]n = 77.9
13n = 77.9
Divide both side by 13
n = 77.9 / 13
n = 6
Molecular formula = [CH]n
Molecular formula = [CH]₆
Molecular formula = C₆H₆
Complete Question:
0.265g of an organic compound produced on evaporation 102cm cube of vapour at 373K and 775mmHg. Percentage composition of the constituent elements are 92.24% C and 7.76% H. Find the molecular mass and molecular formula of the composition.
Learn more about ideal gas equation:
https://brainly.com/question/14364992
Learn more about molecular formular:
https://brainly.com/question/512891
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