Orgo Experiement 1
CHM 2210L-009
Experiment 1: Simple and Fractional Distillation of a Binary Mixture
Aim: The aim of this experiment is to perform a simple and a fractional distillation and separate a mixture containing two liquids, cyclohexane and toluene.
Post Lab:
At any given temperature a liquid is in equilibrium with its vapor. This equilibrium is described by the vapor pressure of the liquid. The vapor pressure is the pressure that the molecules at the surface of the liquid exert against the external pressure; this is usually the atmospheric pressure. Vapor pressure does not increase linearly but instead, increases exponentially with temperature. The vapor pressure of a substance roughly doubles for every increase in 10 °C. When the vapor pressure of the liquid equals the applied pressure, the liquid boils. Therefore, the boiling point of a liquid is the temperature at which the vapor pressure equals the applied pressure. The normal boiling point of a liquid is the temperature at which the vapor pressure of a liquid equals atmospheric pressure, which is about 1 atm. The boiling point of a liquid is a measure of its volatility.
There are two types of distillations used in this experiment. The first method is simple distillation. This process is the simplest method and sometimes does not provide acceptable results. Simple distillation is most valued when only one of the compounds in the binary mixture is volatile, thus the volatile compounds distills out leaving the nonvolatile compound behind. Simple distillation requires a large discrepancy between boiling points of the compounds (≥40-50oC) to be separated to gain meaningful purity of the distillate.
The second method that was used is fractional distillation. This method works in principle the same as simple distillation but adds a distillation column between the vial and the condenser. The distillation column is hotter at the bottom and cooler at the top. As the vapor passes
Experiment 1: Simple and Fractional Distillation of a Binary Mixture
Aim: The aim of this experiment is to perform a simple and a fractional distillation and separate a mixture containing two liquids, cyclohexane and toluene.
Post Lab:
At any given temperature a liquid is in equilibrium with its vapor. This equilibrium is described by the vapor pressure of the liquid. The vapor pressure is the pressure that the molecules at the surface of the liquid exert against the external pressure; this is usually the atmospheric pressure. Vapor pressure does not increase linearly but instead, increases exponentially with temperature. The vapor pressure of a substance roughly doubles for every increase in 10 °C. When the vapor pressure of the liquid equals the applied pressure, the liquid boils. Therefore, the boiling point of a liquid is the temperature at which the vapor pressure equals the applied pressure. The normal boiling point of a liquid is the temperature at which the vapor pressure of a liquid equals atmospheric pressure, which is about 1 atm. The boiling point of a liquid is a measure of its volatility.
There are two types of distillations used in this experiment. The first method is simple distillation. This process is the simplest method and sometimes does not provide acceptable results. Simple distillation is most valued when only one of the compounds in the binary mixture is volatile, thus the volatile compounds distills out leaving the nonvolatile compound behind. Simple distillation requires a large discrepancy between boiling points of the compounds (≥40-50oC) to be separated to gain meaningful purity of the distillate.
The second method that was used is fractional distillation. This method works in principle the same as simple distillation but adds a distillation column between the vial and the condenser. The distillation column is hotter at the bottom and cooler at the top. As the vapor passes