You distilled a mixture whose composition was known on a vol : vol basis. Howeve

Question

You distilled a mixture whose composition was known on a vol : vol basis.
However, molar composition is usually more useful. Apply the data below to a 15.0 mL
sample consisting of: 30% 2-propanol, 30% chloroform and 40% octane
* Chloroform (CHCl3): formula mass: 119.38 g/mol; density: 1.48 g/mL; bp: 61.7 C
* 2-propanol (C3H8O): formula mass: 60.11 g/mol; density: 0.786 g/mL; bp: 82.4 C
* Octane (C8H18): formula mass: 114.23 g/mol; density: 0.702 g/mL; bp: 125.7 C

Mass octane: 4.212 grams
Mass % of octane: 29.232 %
Moles of Octane: 0.036883 moles
Moles % composition: 24.34%

Mass Chloroform: 6.66 grams
Mass % of chloroform: 46.22111%
moles of chloroform: 0.055788 moles
Moles % composition: 36.82%

Mass of 2-propanol: 3.537 grams
Mass % of 2-propanol: 24.547 %
moles of 2-propanol: 0.058842
Moles % composition: 38.84 %


My questions are:
1.) How would you sketch the theoretical curve expected for the distillation of 12.0 mL of the
15.0 mL of the ternary mixture described above?

2.) Also how would you use an experimental distillation curve to determine the %,
by volume, composition of an unknown mixture?

Explanation / Answer

You distilled a mixture whose composition was known on a vol : vol basis. Howeve

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