The PreLab Exercise A mixture of 40 mL of methyl butyrate (MW=102.1 g/mol, d=0.8

Question

The PreLab Exercise A mixture of 40 mL of methyl butyrate (MW=102.1 g/mol, d=0.89 g/mL) and 10 mL butyric acid (MW=88.1 g/mol, d=096 g/mL) is distilled. Calculate the mole percent of each component, and using these mole percents and the figure below, answer the following questions: 1. What is the initial boiling point of this mixture? 2. What is the composition of the vapor In equilibrium with this liquid? What is the composition of the initial condensate from simple distillation? 3. Instead of a simple distillation, you set up a fractional distillation. Assuming three theoretical plates, what is the composition of the first fraction collected?

Explanation / Answer

Volume of methyl butyrate = 40 mL

Density of  methyl butyrate = 0.89 g/mL

Mass of  methyl butyrate = 40*0.89

= 35.6 g

moles of methyl butyrate = 35.6 / 102.1

= 0.348

Volume of butyric acid = 10 mL

Density of butyric acid = 0.96 g/mL

Mass of  butyric acid = 10*0.96

= 9.6 g

moles of butyric acid = 9.6 / 88.1

= 0.108

mole percent of methyl butyrate = 0.348 / (0.348 + 0.108) * 100

= 76.32%

mole percent of butyric acid = 0.108 / (0.348 + 0.108) * 100

= 23.68%

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