...Taking your three tubes, place each alcohol in them separately and add 1ml of cyclohexane. 2. Rattle the test tube gently to see if there is any change and evidence of miscibility within the tubes. 3. Repeat the first and second step but instead of using Cyclohexane, replace it with water. \ 4. In the mixture with Cyclohexane, and in the mixture of water, take litmus paper and record the color change shown. 5. Dispose the contents carefully and with care along with notifying your supervisor and/or teacher. Observations/ Results Alcohol Name Structural diagram Melting point Boiling point Solubility in cyclohexane Solubility in water Color with yellow/orange litmus paper Propanol -127 degrees Celsius 97 degrees Celsius soluble Not soluble yellow orange butanol -90 degrees Celsius 117 degrees Celsius soluble Not soluble yellow Orange Ethanol -114 degrees Celsius 78 degrees Celsius Insoluble Soluble yellow Orange From the observations recorded, after the solutions have been mixed with each other the results show that...
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...the conversion of a solvent into a vapor then back to a solvent based on vapor pressure. The liquid with the lowest boiling point and highest vapor pressure would be collected first (Weldegirma,2017). There are various distillation methods, however the two methods utilize in this experiment are: simple and fractional using cyclohexane and Toluene. Simple distillation is more efficient when the boiling points are more than 25℃ difference and fractional distillation is more effective in separating liquids with boiling point less...
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...At room temperature, there is a rapid equilibrium between the two chair conformations of cyclohexane. The twist-boat and chair are both energy minima—the twist-boat being a local minimum and the chair being a global minimum (ground state). The energy of twist-boat conformation is 5.5 kcal mol−1 (23 kJ mol−1) higher than that of the chair conformation. The half-chair state (2, below) is the transition state in the interconversion between chair and twist-boat conformations. Because of the D2 symmetry of the twist-boat, there are two energy-equivalent pathways that it can take to two different half-chair conformations, leading to the two different chair conformations of cyclochexane. Therefore, at a minimum, the interconversion between the two chair conformations involves the following sequence: chair - half-chair - twist-boat - half-chair' - chair'. The energies of boat and half-chair states are 6.5kcal mol−1 (27 kJ mol−1) and 10kcal mol−1 (42 kJ mol−1) higher than that of the chair. The conformations involve following stability order: chair form > twist boat form > boat form > half-chair form....
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...ABSTRACT Nylons comes in many types but the most common and widely used in textile and plastic industries are Nylon 6 and Nylon 6,6. Nylon 6,6 is made up of two monomers each containing 6 carbon atoms. One of them is Adipic Acid which is a dicarboxylic acid. It is manufactured by oxidation of Cyclohexanol which is produced by oxidative cleavage of cyclohexane or by hydrogenation of phenol. Commercially Cyclohexane is preferred as raw material because of its lower cost and a two-step mechanism involving Nitric acid is used to produce Adipic Acid. This process has higher selectivity and yield than other processes. The only concern with this process is the emission of nitrogen oxides in the gas effluents which is a major environmental concern. 1. Introduction Adipic acid is an organic compound, with formula HOOC (CH2)4COOH, which is a white crystalline solid and one of the most important Dicarboxylic acid. It is Odorless, Colorless and freely soluble in Ethanol, Methanol and Acetone. Other Important properties of Adipic acid is shown in Table 1.From Industrial perspective it is used mainly in Nylon-6, 6 production. About 2.5 billion kilograms of this white crystalline powder are produced annually. In US it is mainly produced by three companies at four manufacturing plants, with nearly two-thirds of the total production, 860,000 tons capacity occurring at DuPont's two Texas facilities. The use of adipic acid in food items have started in recent times and this has created a demand...
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...was to witness the change in temperature of cyclohexane with different substances added. The process of phase change is usually being witnessed in the different weather changes we have. When snow begins to fall in the winter it falls as a liquid, starts to freeze from the atmosphere, then fully freezes when it is set on the ground from the winter temperature. It then begins to melt and turn back into a liquid as the temperature begins to heat up, then evaporates as the liquid starts to boil and steam up. (Phase Change, 17). In this experiment, we hypothesized that our trial three with 0.612 grams of benzoic acid would have the greatest effect on temperature change since it held the greatest...
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...mixture of cyclohexane and toluene were separate from one another by fractional distillation in order to measure the composition of each fraction and prepare the sample for gas chromatography. Introduction: Distillation has been used since antiquity to separate the components of mixtures. This method has been used to manufacture different organic chemicals but the most recent application is the refining of petroleum in order to produce fuels, lubricants and petrochemicals. In this experiments, the separation of 2 distilates were carried out using the differences in boiling points and the data was used for a gas chromatography test. Objectives: Separation of an equimolar mixture of cyclohexane and toluene by fractional distillation Materials: Equimolar mixture: cyclohexane/toluene Water Distilling columns Column packing Thermometer heat source flasks heat source Structural Formulas: toluene Description: The fractional distillation apparatus was checked for any moisture before it was set up to ensure proper distillation method. A mixture of cyclohexane and toluene was obtained, 40ml of an equimolar mixture was obtained and transferred into a 100ml round bottomed boiling flask which contained boiling chips, and the distilling column was packed with metal sponge. The distillation apparatus was assembled and a heat mantle was set and several vials were used as fraction receivers and labeled 1-5. The cyclohexane/toluene...
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...Laboratory Questions: 1,2,3,4, and 5 1. Part A.3. Some of the cyclohexane solvent vaporized during the temperature versus time measurement. Will this loss of cyclohexane result in its freezing point being recorded as too high, too low, or unaffected? Explain. If some of the solvent has vaporized, the freezing point in part A.3. will not be affected because in that step the cyclohexane is still a pure substance without a solute to lower its freezing point (Beran, 2014). 2. Part A.3. The digital thermometer is miscalibrated by +0.15°C over its entire range. If the same thermometer is used in part B.2 will the reported moles of solute in the solution be too high, too low or unaffected? Explain. Because of the miscalibrated thermometer being used for each part of the experiment, the calculation for the reported moles of the solute will remain unaffected because the calculations only take the overall change of the freezing point into consideration, not the freezing point itself (Beran, 2014)....
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...So far, we’ve only talked about cyclic molecules containing one ring. But, of course, molecules with multiple rings are very common in nature. A prime example is the steroid structure, exemplified by the common oral contraceptive ethinyl estradiol. estradiol Here, we’re just going to talk about two very simple cases of molecules containing two rings. We’re going to focus our efforts on cyclohexane, and examine in close detail the situation where two cyclohexane rings are bonded to each other in the most common way – with the two ring junctions (“bridgeheads”) on adjacent carbons, a situation we refer to as fused rings. The parent molecule is called “decalin” since there are ten carbons in total. However, remember that any time we have two substituents on a cyclohexane ring (as we do here), it is essential to draw in the stereochemistry in order to avoid ambiguity! Two stereoisomers are possible here: one where the hydrogens at both ring junctions are “cis”, and the other where they are “trans”....
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...In the cyclohexane molecule all of the hydrogens are staggered and because the atoms are closer than 2.40 Angstroms apart, steric strain exists between the carbon hydrogen bonds. Overall, cyclohexane is a very stable molecule, which is shown by its low energy and low steric strain. Cyclopropane is a very unstable molecule because it has steric and torsional strain and a high energy. The chair conformation of cyclohexane is the most stable form of cyclohexane. This is because it has the lowest energy due to having minimal steric strain caused by the distance of the hydrogen atoms. The boat conformation of cyclohexane is less stable than the chair form of cyclohexane because it has a higher energy due to the eclipsed hydrogen bonds. The hydrogen bonds are generating steric strain due to hydrogens being in the same plane. The axial axial 1,2-dimethylcyclohexane is the least most stable configuration, followed by This is because axial bonds are less stable than equatorial bonds due to less strain on the molecule. This conclusion can be applied to all molecules in cyclohexane...
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...Mlungisi Maphunta 147565 Bachelor of Science II C202 Practical Report Group 15 Experiment8 COLLIGATIVE PROPERTIES: FREEZING POINTDEPRESSION AND MOLAR MASS Group Members Mncedisi Mngomezulu Sphiwe ndwandwe Thandeka Mpila EXPERIMENT 8: COLLIGATIVE PROPERTIES: FREEZING POINT DEPRESSION AND MOLAR MASS: AIM The aim of the experiment is to become familiar with the colligative properties and to use them to determine the molar mass of a substance. THEORY A solution consists primarily of solvent and therefore, most of the solution’s properties reflect the solute’s properties. The physical properties that the solution and solute do not share are known as colligative properties and they depend solely on the solute concentration. Some of these properties include vapor pressure lowering, boiling-point elevation, freezing point lowering, and osmotic pressure. The solvent boils when the vapor pressure, or tendency of solvent molecules to escape, is equivalent to the atmospheric pressure. At this moment, the gaseous and liquid states of the solvent are in dynamic equilibrium and the molecules change from the liquid to the gaseous states and from the gaseous to liquid states at equal rates. The dissolution of a solute with very low vapor pressure, or a nonvolatile solute, raises the boiling point and lowers the freezing point. Similarly, anti-freeze lowers the freezing point and lowers the boiling point. The colligative-property law describes these effects, stating that the "freezing point...
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...STEEL WOOL STEEL WOOL STEEL WOOL BEADS BEADS BEADS BEADS Sample 1.4661 1.4615 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 1.4661 First Second Mole Fractions Residual 1.4437 1.4405 1.4516 1.4476 1.4845 1.4780 1.4380 1.4402 1.4451 1.4354 1.4360 1.4701 1.4475 1.4430 1.4325 1.4355 1.4380 1.4350 1.4375 1.4375 1.4388 1.4326 1.4358 1.4340 1.4369 1.4380 1.4455 1.4480 1.4410 1.4433 1.4545 1.4505 1.4380 1.4440 1.4370 1.4455 1.4760 1.4815 1.4815 1.4777 1.4814 1.4885 1.4877 1.4821 1.4900 1.4905 1.4924 1.4785 1.4865 1.4820 1.4899 Sample First Second Residual Cyclohexane Toluene Cyclohexane Toluene Cyclohexane Toluene Cyclohexane Toluene 0.44 0.56 0.75 0.25 0.64 0.36 0.18 0.82 0.50 0.50 0.80 0.20 0.70 0.30 0.27 0.73 0.44 0.56 0.83 0.17 0.86 0.14 0.30 0.70 0.44 0.56 0.80 0.20 0.38 0.62 0.22 0.78 0.44 0.56 0.73 0.27 0.70 0.30 0.22 0.78 0.44 0.56 0.87 0.13 0.76 0.24 0.27 0.73 0.44 0.56 0.91 0.09 0.83 0.17 0.22 0.78 0.44 0.56 0.87 0.13 0.73 0.27 0.12 0.88 0.44 0.56 0.83 0.17 0.69 0.31 0.13 0.87 0.44 0.56 0.88 0.12 0.79 0.21 0.21 0.79 0.44 0.56 0.84 0.16 0.76 0.24 0.10 0.90 0.44 0.56 0.84 0.16 0.60 0.40 0.09 0.91 0.44 0.56 0.82 0.18 0.66 0.34 0.06 0.94 0.44 0.56 0.91 0.09 0.83 0.17 0.26 0.74 0.44 0.56 0.86 0.14 0.75 ...
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...Purpose The purpose of this experiment is to determine the energy level diagram of anthracene using its absorption and fluorescence spectra, as well as the quantum yield and rate constant of fluorescence quenching of antracene by CCl4. Methods A solution of anthracene and another solution of CCl4 are made in ethanol and mixed and diluted to various concentrations. The fluorescence and absorption spectra of these solutions are measured using a UV-visible spectrometer and a fluorescence spectrometer. Then a solution of anthracene is prepared in cyclohexane. Again, the fluorescence and absorption spectra are obtained and served as a reference for all calculations. Procedure The procedure followed was given in the lab manual, Experiment 23,...
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...Azeotropic Distillation of water and ethanol by Harold van Schevensteen The process of simple distillation is a method of separating mixtures based on their differences in volatility in a boiling liquid mixture. We find out, however, that using this process, a mixture of water and ethanol cannot be separated fully. The latter can only be purified to approximately 96%. To get to this point, we go through a process whereby through distillation, we reduce the proportion of water in the mixture and increase that of ethanol. For example, if we were to distill a 50/50 mixture of ethanol and water, the distillate would be 80% ethanol and 20% water. Distilling this new mixture produces a mixture of 87% ethanol and 13% water. This goes on until we reach a ratio of 95.63% ethanol and 4.37% water, at which we reach a point called the azeotropic point of the mixture. At this stage, the mixture is called a positive azeotrope, which is defined when the ratio of the constituents cannot be further changed by simple distillation. This occurs because any further boiling of the mixture will result in a vapour who’s ratio of constituents is the same as the original mixture. The closer we get to this point, the lower the boiling point of the mixture as a whole. Ethanol has a boiling temperature of 78.4°C and water one of 100°C. When we have reached the azeotropic point, the mixture as a whole boils at a temperature of 78.2°C. Any further distillation will see the azeotrope boil at...
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...A miniscale diels-alder reaction was performed between the conjugated diene 2,3dimethyl-1,3 butadiene and a substituted alkene such as maleic anhydride in order to produce a substituted cyclohexane. The substituted cyclohexane produced was 4,5-dimethyl-4-cyclohexene-cis-1,2-dicarboxylic acid anhydride. A diels- alder reaction does not have an intermediate state, meaning that bond breaking and bond making occurs at the same time. Heat needs to be applied in order for the reaction to occur and it is very important that 2,3 dimethyl-1,3 butadiene to be cis otherwise there will not be an reaction. During the experiment the melting point of the final product was recorded to be 88°C which is higher than the theoretical melting point of 78-79°C. A low melting point indicates impurities in the purified product where as a higher melting point could be a result of heating the sample too fast. Another error could have occurred from placing too much sample in the capillary tube while performing the recording of the melting point....
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...3. INTRODUCTION Organic compounds are isolated either from natural sources or from reactions mixtures. These compounds are seldom pure and are usually contaminated with small amounts of other similar compounds, which are found to exist together or formed during the reaction. In order to characterize them, it is important to purify them. 4. PROCESSES FOR PURIFICATION 1. Crystallization 2. Sublimation 3. Distillation 4. Chromatography 5. Differential Extraction 6. Qualitative Analysis 5. 1. CRYSTALLIZATION Aim To separate a solid compound in pure and geometrical form. Principle A saturated solution of the impure substance in a suitable solvent is made at a temperature higher than the room temperature. On cooling this solution, the substance reappears in the form of well shaped crystals. Process Purification by crystallization involves the following steps: Choice of solvent Preparation of solution Filtration of the solution Separating the crystals Drying of crystals Example Crystallisation of Phthalic acid 6. 2. SUBLIMATION Aim To separate volatile solids, which pass directly into vapour state on heating from a non-volatile solid. Principle A mixture of solid substances, such as camphor, benzoic acid, ammonium chloride, iodine etc., containing non-volatile substances, when heated, change directly into vapour without passing through the liquid state. Process 7. Fig :-Sublimation 8. 3. DISTILLATION Aim To separate a solution of a solid in a liquid and for separating a solution...
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