Cyanuric Chloride Lab Report

The percent composition of Oxygen and Potassium Chloride in Potassium Chlorate was calculated by heating the compound in a crucible making the Oxygen evaporate as a gas. Silver nitrate tests were conducted with the residue to verify that the residue was potassium chloride. The starting mass of KClO3 was weighed at 1.259 grams. The mass of residue in the crucible after heating was 0.506 grams. This concludes that the mass of Oxygen that was in the KClO3 was 0.753 grams. The percent by mass of Oxygen in KClO3 was calculated at 59.81% while the theoretical percent was 36.166%.

A unimolecular nucleophilic substitution of t-amyl alcohol should be done to convert into t-amyl chloride through extraction and simple distillation. A concentrated hydrochloric acid was added to the reactant to force the reaction to take place. Infrared spectroscopy was utilized to verify that the contents of the tert-amyl chloride should be different from the starting material.

The methyl free radical attack another chlorine molecule to form chloromethane and a chlorine free radical.

Also if precipitate is formed or supernate record that in data table. 8. When this reactions happens this forms two new compounds. Enter in data table. 9.

The melting point found for tran-cinnamic acid in part 1 as well as all 3 of the compounds tested in part 2B fall in this range. The melting point found for the unknown compound (which was identified to be trans-cinnamic acid) is only slightly higher than the range. This can be due to errors such as an error in the software or not recording the temperature immediately after the last crystal liquefied. Overall, the results found in this experiment support the data found on

In 1788 Charles made his own bleaching field, and by 1799 had made chloride of lime. Chloride of lime is another term

The product of this reaction is an aromatic molecule, which can be activating or deactivating. An aromatic ring with an oxygen sigma bonded to C1 and a methyl group is considered activating. This molecule is activating because the oxygen has two lone pairs of electrons surrounding it. In contrast, an aromatic ring with a carbon sigma bonded to an aldehyde is considered deactivating. This is due to the double bond of the oxygen to the carbon. Another observation seen in this reaction were emulsions. These were seen because water and HCl were added to the solution. Both serve as salts in this instance, as they both want to dissociate in both layers. In order to solve this issue and get the most product, sodium bicarbonate was added to the solution.

20) The reaction Cl-l3CH3 + Br2 - CH3CH2Br + r!Br would best be described as:

Atomic and Molecular Properties Atomic Symbol - Cl Atomic Weight - 35.453 Atomic Number - 17 Molecular Weight of Cl2 - 70.906 Physical properties Physical Properties Property Definition Conditions Value Boiling Point (Liquefying Point) The temperature at which liquid chlorine vaporizes 14.696 psia (101.325 kPa) -29.15° F (-33.97°C) Critical Density The mass of a unit volume of chlorine at the critical pressure and temperature 35.77 lb/ft3 (573.0 kg/m3)

Bis(2-chloroethy1)aminophosphoric dichloride (73.5g, 28.4mmol) is dissolved in THF (150mL).6 A solution of 3-aminopropanol (21.3g, 28.4mmol) is dissolved in a separate bath of THF (150mL), and triethylamine (79.0mL) is added.6 These two solutions are simultaneously added dropwise into stirred dry THF (300mL) over 3 h.6 Once both of the solutions have been added, the reaction is left overnight at room temperature, with continuous stirring.6 The resulting solution is then vacuum filtered as to remove the Triethylammonium hydrochloride, and the filtrate will evaporate under vacuum.6 The remaining residue is then subject the silica gel chromatography (100g), with chloroform-methanol.6 This should result in a colourless oil, which is dried under vacuum over P401o. The dried substance is then recyrstallised from dry ether at -78oC.6 This chemical synthesisV was reported by Verkade in 1978. Verkade and his research team reported a yield of

The intention to enhance the databank of the structure activity relationships of benzalkonium by using chloride as a cation structure in order to determine the stability. To help resolve the problem the only thing to do is to attempt renewed structures so that one can examine what activity they will result in. In the synthesis of group one compound they have polar and non-polar elements which can be perceived how this affects the activity of the structure. In the synthesis group one compound there appears to be a large quantity of OH groups and from recognizing one can see that the OH can interact with the cell causing it to absorb light. The general synthesis starting compound appears to be strained and open in order to interact with R1, R2, and NH. The results of the general synthesis transpired as a salt that is a solid but when Saad had gotten his results he got a formation of a liquid instead of a solid. Now Saad has to synthesize the compound in order to see if he will get a solid instead of another

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CuCl is used a catalyst and a green solvent, 2-propanol, is also used as a reaction medium which is a greener solvent. Results/Discussion:

This chemical reaction was discovered in 1828 by Friedrich Wohler in an attempt to synthesize ammonium cyanate. It is considered the starting point of modern organic chemistry. Wohler wanted to prove, contrary to scientific thinking of the time, that a product of the living processes of animals could be made in the laboratory from inorganic materials. The synthesis was almost an accident, as Wohler had been trying to make another compound, ammonium cyanate, to continue a study of cyanates he had been working on for the previous few years. When he added silver cyanate to ammonium chloride solution he obtained a white crystalline material, which proved identical to urea obtained from urine.

A pure compound can be identified by specific physical properties such as its melting point. A compounds melting point varies depending on how pure the compound is, a higher melting point indicates a more pure compound. The purpose of this experiment is to determine the melting point of given crystalline substances as well as the identity of an unknown substance based on its melting point. The DigiMelt melting point apparatus is used in this experiment to determine melting points of different crystalline substances by allowing one to view the substances during the melting process. In part 1 of the experiment, the melting point ranges for Urea, Trans-Cinnamic Acid, and a 50:50 mixture of the two were found to be 4.4, 3.1, and 31.6 respectively.