Cyclohexanone Lab Report

The reaction mixture was created. Tetraphenylcyclopentadienone (0.1197g, 0.3113 mmol) a black solid powder, anthranilic acid ( 0.0482g, 0.3516 mmol) a yellowish sand, and 1,2-dimethoxyethane (1.2 ml) was added to a 5-ml conical vial. A spin vane was added and a water-jacked condenser was attached. Isopentyl nitrite (0.06ml, 0.045 mmol) was dissolved in 1,2-dimethoxyethane (0.50 ml) in a 3-ml conical vial and caped to prevent loss by evaporation.

Dehydration reactions are important processes to convert alcohols into alkenes. It is a type of elimination reaction that removes an “-OH” group from one carbon molecule and a hydrogen from a neighboring carbon, thus releasing them as a water molecule (H2O) and forming a pi bond between the two carbons1. In this experiment, 2-methylcyclohexanol undergoes dehydration to form three possible products: methylenecylcohexane, 1-methylcyclohexene, and 3-methylcyclohexene in a Hickman still apparatus. Adding 85% Phosphoric Acid to protonates the “-OH” group, turning it into a better leaving group and initiating the dehydration reaction. The dehydration of 2-methylcyclohexanol takes place at the bottom of the Hickman still. As the Hickman still heats up within the sand bath, the products evaporate and travel higher up in the still where they condense into a liquid and fall within the collection ring, thus separating the product from the remaining water. Drierite (CaSO4) is also added as a drying agent to absorb any leftover water within the product. The purity of the product will then be analyzed with infrared spectroscopy, paying attention to OH peak if it is present.

Because the heating block readily increased in temperature, the temperature had to be adjusted accordingly to prevent the overheating the reaction. Initially, the color of the reaction turned into a dark green color and over time became a lighter shade with a minimal solid left. The reaction process lasted for 2 hours. As the reaction heated for 2 hours, a 50 mL beaker was weighed, approximately 12 mL of 20% ethyl acetate in hexane solution was added to a 25 mL Erlenmeyer flask, and 2.0 mL of saturated NaCl solution was added to a labeled test

When the aqueous layer was added to the vial, calcium chloride was then added to dry the solution. If the solution was dry enough, a large peak between 3300-3500 would have been present in the IR spectrum. In order to obtain the IR spectrum two Classification test were performed. The Bromine test and Permanganate test were used to determine if alkenes were indeed present in the solution. Both test were positive for the compound. During the Bromine test, the bromine transformed from brown to clear indicating the presence of an alkene. Also during the permanganate test, the compound changed from purple to brown. This also indicates the presence of an alkene, which indicates the E2 reaction did occur. These two positive test allowed for a GC spectrum to be obtained, if the IR confirmed there was no water in the final compound. The IR spectrum obtained, did contain a peak at 3388 cm-1, indicating an alcohol group present, but the degree of the peak was so small that a GC spectrum could be obtained. This peak could have represented water present in the solution, but its presence was so low that it would not affect the

The purpose of this lab experiment is to examine different types of chemical reactions such as Decomposition reaction, Synthesis reactions, Combustion reactions, and different Chemical equations. The experiments were conducted online using Late Nite Labs.

In this experiment, a balanced chemical equation will be provided for decomposition reactions. A redox reaction is a reaction where one reactant is reduced due to a gain of electrons, and the other is oxidized due to a loss of electrons. The reactant that loses an electron is called the reducing agent, whereas the reactant that gains an electron is called the oxidizing agent. In this experiment, the balanced chemical equation, and the two half equations for the redox reactions will be provided, and the oxidizing and reducing agents will be

The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield. Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated

K.D.A. Saboia et al., (2007) have been prepared the Bi4Ti3O12–CaCu3Ti4O12 {[BIT(X)–CCTO(100-X)]} composite powders through solid state reaction method and calcined in the range of 900 to 1020 ºC for 12 h. The as-prepared powders have modified in the form of thick film onto alumina ceramic substrate by utilizing screen printing. At 100 Hz, the value of dielectric constant (κ) of CCTO100 and BIT100 is 316.61 and 53.64 respectively. Conversely, the composite with X=20 % shows an unexpected dielectric constant of 409.71, which is around 20% higher in comparison with the CCTO. These measurements strongly suggest that the BIT–CCTO composite are good candidates for applications where one search for high-κ materials with low loss in radio-frequency range.

The purpose of this experiment was to perform a bromination reaction that converts cyclohexane to trans-1,2-dibromocyclohexane. To do this, 1 mL of 30% hydrogen peroxide was mixed with 3 mL of bromic acid in a round bottom flask containing a spin vane. The solution turned from clear to orange, dark red. The color change is a useful indicator to identified whether reaction was completed before moving to another step. Next, 1 mL of cyclohexene was pipet into this mixture, which changed the solution from red to orange and eventually yellow. The mixture was transferred into a centrifuge tube with brine solution. Two layers were formed, with a yellow layer on top and the clear bottom layer. The bottom layer is the only organic layer because it is denser. NaHSO3 was used to washed the mixture. The bottom layer was extracted by pipette and rinsed with NaSO4 for drying. The organic layer was transfer into a vial and placed under NEVEP to attain a solid product. The product was a mixture of white solids with liquid.

To begin the experiment, 50 mg of 4-t-butylcyclohexanone and methanol were added to a conical vial. NaBH4 was then added to the reaction mixture to reduce the ketone functional group (present in the starting material). The reaction was allowed to proceed for 30 minutes and was subsequently quenched using hydrochloric acid. The addition of hydrochloric acid permitted the protonation of the reduced ketone (O-) to form the two diastereomer

Strong acids and strong acids both dissociate completely in water forming ions. However, strong acids donate a proton to form H3O+ along with a conjugate base and strong bases accept a proton to form OH- along with a conjugate acid. The chemical behavior of acids and bases are opposite. When they are together, their ions cancel out and form a neutral solution. In this experiment, HCl and NaOH will react to form NaOH and H2O with these two steps:

Chevron Phillips Chemical Company is the major producer of Cyclohexane. This successful company hoses the three largest cyclohexane plants in the world. Many are puzzled by how the production of cyclohexane seems to have become stagnant. Perhaps this is due to the cost of benzene increasing or the demand increasing. Through thorough investigation, the answer to this question and many more can be answered. There are two methods of obtaining cyclohexane. These two methods are fractional distillation of naphtha and hydrogenation of benzene. Research suggest that the hydrogenation of benzene is the most economical way to create our chemical of choice. According to ICIS, cyclohexane is used in the production of adipic acid used to

The unknown concentration of benzoic acid used when titrated with standardized 0.1031M NaOH and the solubility was calculated at two different temperatures (20◦C and 30◦C). With the aid of the Van’t Hoff equation, the enthalpy of solution of benzoic acid at those temperatures was determined as 10.82 KJ. This compares well with the value of 10.27KJ found in the literature.

In 1937, the German scientist “prof. Otto Bayer” and his co-workers was find out the poly addition reactions1-4 where the polyaddition of diols and diisocyanates in the presence of catalyst to proceeds completely to forms a polyurethanes (PUs) in the presence of mild conditions to avoid the undesired by products. Hence, prof. Otto Bayer was recognized as a “father” of polyurethanes. At the time of during World War II, for aircraft coating purpose in small-scale PUs was used but that time polyisocyanates not available in market. After that the World War II, some research groups focused on their activities and interests in PUs establishment in various countries like U.S.A and U.K but the commercial development is very slow. However, the German

Define SPE and explain the role of each of the steps used to prepare the SPE cartridge for the isolation of the analyte.