Wait a second!
More handpicked essays just for you.
More handpicked essays just for you.
Experiment with fraction distillation
Simple distillation discussion
Fractional distillation of binary liquid solutions
Don’t take our word for it - see why 10 million students trust us with their essay needs.
Recommended: Experiment with fraction distillation
Title: Distillation of Cyclohexane and Toluene
Introduction: The experiment was conducted to show which type of distillation is the most accurate in separating the two liquids. Simple distillation results were compared to the different techniques of fractional distillation in order to show which was the most accurate in separating the liquids.
Procedure: This experiment followed the directions present in the manual for the simple distillation method. 15 mL of the Cyclohexane and Toluene solution was used in the distillation flask and the heating mantle was initially set at 25V. Eventually, our TA suggested to turn up the heating mantle to 50V because the liquid was not boiling after 20 minutes of heat. After the forerun was disposed,
…show more content…
For the first fraction, it was collected at temperatures between 79oC and 95oC. Based on the boiling point of Cyclohexane being 80.7oC and the boiling point of Toluene being 111oC, the first fraction should have been almost completely composed of Cyclohexane. The second fraction was collected at temperatures between 95oC and 100oC and should have been mostly composed of Toluene because the majority of the Cyclohexane should have been in the first fraction. Since the residual liquid was the liquid that had not boiled at a temperature of 100oC, then almost all of that remaining liquid should have been …show more content…
The average mole fraction for the different types of fractional distillation with packing is less than 0.15; the fractional distillation packed with steel wool had the lowest mole fraction at 0.1386139 and the simple distillation set up had the highest mole fraction at 0.336633663. In the second fraction the mole fractions varied significantly between the different setups. The fractional distillation with steel wool had the lowest average at 0.5293501, while the fractional distillation with the empty column had the highest average at 0.821075. The fractional distillation with beads (mole fraction of 0.7008487) and rings (mole fraction of 0.7095746) had very similar average results, while the simple distillation had a mole fraction of 0.557708628. In the residual fraction, which was supposed to be almost pure Toluene, all of the distillation setups had mole fractions of Toluene above 0.94. The fractional distillation with the empty column had the highest average mole fraction with 0.97843 and the fractional distillation with the steel wool had the lowest average mole fraction with 0.9466054. While the fractional distillation with the empty column had the purest residual liquid remaining, the individual data points for all the
Methanol, acetone, dichloromethane, toluene, and hexanes were tested for their miscibility with water. Methanol and acetone were found to be miscible with water, and dichloromethane, toluene, and hexanes were immiscible. Two layers—one organic and one aqueous—were observed each time an immiscible solvent was combined with water. Dichloromethane was observed as the bottom layer, and toluene and hexanes were observed as the top layers when added to test tubes of water. In Table 1 below, density, boiling point, and miscibility with water are shown for the organic solvents used in this experiment.1
The mass of 2mL of the solvent, p-xylene, was measured as well as the mass of 10 drops of toluene, the solute. The temperature of the solution rose to the freezing point after supercooling, then continued to drop as the solution froze, versus stabilizing as the pure p-xylene did. The maximum temperature obtained after supercooling was recorded as the freezing point of the solution. This process was repeated three times, each with a new test tube and the same beaker and scale for measuring the masses, then the Tf was calculated for each trial, as well as the average Kf. For the final portion of the lab, the same procedure as above was followed with the substation of 10 drops of unknown solutes instead of toluene in the p-xylene. Each unknown, A, C, and D, had one trial each. With the experimentally gathered data, the molar masses were then computed and compared to the given compound molar masses to
The objective of this experiment was to use a common method of separation distillation. Distillation can be used in purifying or separating liquids, when the liquid if heated the more volatile component, the molecule with the lower boiling point, vaporizes and can be condensed. This type of separation will work efficiently when the feed mixture has a decent range between the boiling points of the components. The relationship between component’s vapor pressure to the composition of the solution is Ptotal==P1+P2, Raoult’s Law. This can be used with Dalton’s Law of partial pressure,
Use glassware as directed by your instructor. Place a test tube placed inside a beaker with ice water to collect the product from the apparatus. Obtain the 10mL round bottom flask from the apparatus. Obtain two graduated cylinders of 10mL. On one graduated cylinder measure 4mL (85% H3PO4) of Phosphoric Acid and pour into the 10mL round bottom flask. On the other graduated cylinder measure 3mL of Cyclohexanol and pour into the flask as well. With a pipet add 5 drops of Sulfuric Acid (H2SO4) into the flask. Attach the round bottom flask to the distillation apparatus. Place thermometer with rubber stopper on the apparatus to obtain the temperature Start with the water flow through the condenser. Turn on and heat the reaction until the product starts to distill. Distill and collect until thermometer temperature rises to 85˚C. Once there is no more product to collect obtain the test tube of product. Two layers should be formed, top layer of cyclohexane and bottom layer with water. Obtain a pipette and remove the bottom layer (water) if any. Add 10% (5mL) of Sodium Bicarbonate (NaHCO3) to nuclearize any acid in the solution. Mix well and remove once again the bottom layer of water with pipette. Add 5mL of water and mix well to wash the top layer. After the two layers form again, remove entirely the bottom layer of water and add a few pellets of Calcium Chloride. Obtain a 50mL or 100mL beaker and weigh.
Variables --------- During the experiments, the water will be heated using different spirit burners containing different alcohols. I will be able to change different parts of the experiment. These are the. Volume of water heated:
The purpose of this experiment was to learn and preform an acid-base extraction technique to separate organic compounds successfully and obtaining amounts of each component in the mixture. In this experiment, the separation will be done by separatory funnel preforming on two liquids that are immiscible from two layers when added together. The individual components of Phensuprin (Acetylsalicylic acid, Acetanilide, and Sucrose as a filler) was separated based upon their solubility and reactivity, and the amount of each component in the mixture was obtained. Also, the purity of each component will be determined by the melting point of the component.
This experiment required the used of reflux to heat the mixture because it is a technique that does not lose any liquid due to evaporation. A reflux apparatus is capped so that vapors do not escape and the system is contained resulting in a larger end product. The reason for using a distillation technique was to produce an individual component of the starting compound, here 1-propanol and 2-pentanol. Drying is a very important step because if the product is wet, it will have added incorrect water weight. Before drying, first the product must be separated from the organic layer. The reason for applying the reflux method over simple distillation is simply because the reflux is set up to return the condensed distillate to the flask. This allows it to boil, yet lose no solution. Simple
In this experiment, the process of steam distillation was used to purify a natural product, (the essential oil of spearmint). This phenomenon works because when two immiscible liquids are distilled, the boiling point of the mixture is below the boiling point of the both pure compounds. Since water has a significantly lower boiling point than spearmint, a much greater proportion of water molecules was vaporizing at any time during the distillation. Even though the components of spearmint oil have low vapor pressure, they are volatile enough to vaporize to some extent and a small amount will lifted off with the water molecules. This boiling will occur when the independent internal vapor pressures are equal to 760 torr, which is the external vapor pressure. It is noted that steam distillation, unlike regular distillation, it does not follow Raoult’s Law.
The purpose of this experiment is to measure the effect of flow rates on distilled water by recording its volume every second.
Extraction separates compounds based on their solubility. A separatory funnel allows two distinct layers (aqueous and organic) to form when two immiscible liquids are separated with the more dense liquid on bottom. In this lab, dichloromethane (organic) has a density of 1.33g/mL while water (aqueous) has the density of 1.00g/mL, so dichloromethane will be on the bottom and since “like dissolves like” and eugenol does not dissolve in water but dissolves in dichloromethane, eugenol will be found in the dichloromethane layer.
We found that the average density of a full micropipet is 1.03(g/mL). The second table was all about recognizing the density of the unknown. The average density of the unknown is 0.79(g/mL). Table 3 shows the different densities of seven different liquids. Through this table, we discovered that the unknown liquid is ethanol. The density of ethanol is 0.789 which is almost identical to Data Table 2. There could be more options not listed in the table that have a closer density to the unknown.
Determination of concentration of vanilla in this experiment involves three main steps, which are extraction of the vanillin from the other components of the essence using an organic solvent, back extraction of the vanillin as its sodium salt into aqueous phase using dilute sodium hydroxide and determination of the concentration of vanil...
The separation was successful and produced separated stages consistent with prediction based upon solubility properties. This was indicated by the qualitative tests and observations.
fective, cost efficient and environment-friendly process like, simple distillation and study the comparison of different methods present on this field . We aim to reduce the sludge , metals ,dirt and the other volatile matter present in the collected sample of used lubricating oil.
With purer component separation with greater efficiency, distillation is one of promising technique. Investigation on distillation processes found out a number of methods and designs of distillation fitting to different applications. A number of factors that affect the distillation performance and depend upon feed material include distillation column choice, conditions, design parameters, and so on. For instance, vacuum distillation is applied for pressure sensible feed materials, fractional distillation mainly petroleum, while simple distillation to binary mixture of components with different volatilities and so on. The simple binary distillation column sizing method normally involves finding the number of stages from a x-y diagram, the temperature of the distillate and bottoms product using a Txy diagram. The operating lines for the bottom and top of the column depend on the reflux ratio and the condition of the