Abstract — This experiment was conducted to familiarize the students with the procedures regarding distillation—to be more precise, the separation of ethanol from an alcoholic beverage—using a distillation set-up consisting of boiling chips, a Bunsen burner, a condenser, a thermometer and several other materials. In the end, it was discovered that one may actually separate a homogeneous mixture, given that the components of said mixture differ in volatility and that they utilize a complete distillation set-up and follow laboratory safety rules and regulations. Keywords — Matter, homogeneous and hetereogeneous mixtures, distillation, volatility, boiling point I. INTRODUCTION There are typically two categories of matter, these are pure substances …show more content…
II. METHODOLOGY In order to perform this experiment, the students will need a distillation set-up with a connector receiver, an iron ring and stand, a Bunsen burner, a wire gauze, a 250mL round bottom flask, a graduated cylinder, a thermometer, one or two boiling chips, an alcoholic beverage, masking tape, an ice bath, a stirring rod, and, optionally, food coloring. It is imporatnt to avoid playing with the apparatus and equipment so as to avoid breakage and injuries, especially since fire is being dealt with in this experiment. After gathering all of the materials, the experiment can begin. Prepare the distillation set-up similarly to Figure 1[2] and make sure that all of the appropriate areas are secured together with masking tape. In the 250mL round bottom distillation flask, carefully pour in 25mL of the alcoholic bevarage and place in one or two pieces of boiling chips. Now, the students have the option of dyeing the beverage with a tiny drop of food coloring. Afterwards, have the flask sit on the wire guaze on the iron ring and stand and attach it to the distillation …show more content…
Thanks to the boiling chips, the heat is evenly distributed within the flask, which permits a more controlled boil and eliminates the possibility of the liquid in the flask bumping into the condenser[5]. The tedious distillation process is rather simple: the beverage evaporates in the distillation flask and, having no where else to go, enters the condensing tube, where it cools down and is converted back into liquid form. From there on, this liquid flows into the final container, a graduated cylinder [preferably in an ice bath]. The extracted distillate is otherwise known as ethanol, a clear, colorless, flammable liquid, produced through the process of glucose fermentation and frequently used as an intoxicating agent in liquors[6]. In relation to a previous experiment in which the students determined the boiling points of two liquids, it was deduced that the boiling point of [propyl and methyl] alcohol was estimated to be around 80oC. According to numerous sources, ethanol boils (and consequently evaporates) at around 78.5oC[7] a much lower temperature compared to the alcoholic beverage’s other ingredients—water, for example, boils at precisely 100oC. It is immensely possible that because of this, ethanol is isolated from the beverage sooner than said beverage’s other components. Perhaps, if the students worked within
In the first part of the experiment, Part A, the standard solutions were prepared. As a whole, the experiment was conducted by four people, however, for Part A, the group was split in two to prepare the two different solutions. Calibrations curves were created for the standard solutions of both Red 40 and Blue 1. Each solution was treated with a serial 2-fold dilution to gain different concentrations of each solution.
8. Pour 16 oz of room-temperature water into the bottle. 9. Stretch
Characteristic property- Test 1- distillation Materials: Goggles, 250 ml beaker, 10 ml graduated
The Vigreux column has a larger surface area and creates more area for the distillate to condense back into the starting solution. Although the miniscale fractional unpacked distillation is relatively accurate compared to the simple miniscale distillation, the miniscale fractional packed still seems to be the most accurate out of the three. The air condenser in the miniscale fractional packed distillation allows for an extra-added surface area that allows for a greater amount of the liquid to distill separately. The miniscale simple distillation is the least accurate because there is no extra column such as the Vigreux column or the condenser that is added to increase the surface area so therefore any of the vaporized liquid can readily enter the water condenser and condense into the distillate. The 4th technique that was used is called the microscale simple distillation, which is used when there is a relatively small amount of liquid than that used for any of the miniscale techniques.
For this I needed to first obtain deionized water. I cleaned my large graduated cylinder and got 20 + or - 2 mL of deionized water. I then added this water to the beaker that contained the mixture I created from the last step of the experiment. I also gathered 2 boiling stones and added them to the mixture of the last step. I placed the beaker on a hot plate and heated it up to 130 degrees Celsius.
The Effects of Temperatures on Reaction Time of Alka-Seltzer Emily Reynolds October 11, 2015 General Biology Laboratory Northwest Missouri State University Mrs. Heather Meler INTRODUCTION It has been observed that chemical reactions occur at different rates. But, what causes the rates to change? One of the most effective ways to find the answer to that question is through experiments. It has been learned through experimentation that the concentration of a chemical and the temperature can affect the rate of the reaction (Taylor and Mortimer 2002).
Large bubbles with a short duration indicate a higher alcohol content, while smaller bubbles that disappear more slowly indicate lower alcohol content. A common folk test for the quality of moonshine was to pour a small quantity of it into a spoon and set it on fire. The theory was that a safe distillate burns with a blue flame, but a tainted distillate burns with a yellow flame. Practitioners of this simple test also held that if a radiator coil had been used as a condenser, then there would be lead in the distillate, which would give a reddish flame.
Purpose: The purpose of this experiment was to determine the molar mass of unknown #43 using the derived freezing point depression. To obtain the freezing point depression, t-butyl alcohol was placed in a cold-water bath and frozen solid for a total of two runs. Then, unknown #43 was dissolved in t-butyl alcohol and placed in a cold-water bath until frozen solid. This process was repeated for a total of three runs, with the first two runs containing half of the unknown, and the last run containing the full amount of unknown.
Introduction: In this assignment, I will be doing two experimentations on examining the impact of temperature on the Alka-Seltzer’s response time. The first experimentation that I will be doing involves some water that is room temperature. The second experimentation that I will be doing involves some water that is very hot. If I want to be able to figure out the impact of the temperature on water, I will have to document the time it will take for the Alka-Seltzer to go into solution.
Materials and Methods The chemicals used to perform this experiment were distilled water, sodium chloride (NaCl), ice,
The motivation of this investigation was to achieve 85% of methanol recovery from the distillate. II. Methodology: The distillation column was analyzed theoretically using McCabe Thiele to establish the number of stages required for separation. The vapor-liquid equilibrium (VLE) data for methanol and 2-propanol was used to plot curves of methanol-vapor fraction versus methanol-liquid fraction, and methanol liquid-vapor fraction versus temperature.
This includes empty soda can without a top, thermometer, ring stand with iron ring attached, glass rod, 100 ml graduated cylinder, matches, and last but not least two different types of fuel source (propanol, ethanol). Upon completion of the experiment, we got a few notable results. We noticed that the amount of heat absorbed by water is mostly constant between the two but the noticeable difference obtained was with the heat per gram of fuel and heat of
Rediet Legese iLab Week # 6 CRUDE OIL DISTILLATION Introduction: The aim of this week lab experiment is to experiment distill crude oil and to check how temperature determine the chemical properties of crude oil plus how the boiling point can also show physical properties. They are two major finding in this experiment. he first finding was the point at which the raw petroleum is heated to the point of boiling, at 275 0C, the gas and kerosene oil are refined, however the oil (lubricant ) stays as an unrefined feature oil.
Introduction: In this lab, of water in a hydrate, or a substance whose crystalline structure is bound to water molecules by weak bonds, is determined by heating up a small sample of it. By heating, the water of hydration, or bound water, is removed, leaving only what is called an anhydrous compound. Based on the percent water in the hydrate, it can be classified as one of three types: BaCl2O ⋅ 2H20, with a percent water of about 14.57%, CuSO4
This method which uses an internal standard and flame ionisation detector, is exact and more specific than methods usually used. The gas-liquid chromatography method determines ethanol clearly and separately from the other beverage components that would have interfered in other methods, without any distillation or need for a chemical reaction. Determination of ethanol is one of the most vital routine analysis in a current winery. This method provides frequent, rapid and accurate results are needed to regulate the quality of the wine from grape to bottle, as well as for state and federal government