Compare And Contrast The Melting Point Of 4-Butoxyphenyl Acetamide

Melting Point Data Table Compound Aspirin Caffeine Salicylamide Actual MP (ºC) 93 - 98 260 - 262 96 - 102 Expected MP (ºC) 135 236 140 Percent Error (%) ~30% ~12% ~30%

The reaction produces an almost instantaneous

The iodination of O-acetylsalicylamide under the same conditions of this experiment would be slower than Salicylamide, because O-acetylsalicylamide has an amine group, a carboxyl group, and no hydroxyl group, which means that the sodium hypochlorite solution would not be able to deprotonate the Hydroxyl group, thus not allowing a solid precipitate to form, and Hydrochloric acid would not be able to add any Hydrogen atoms due to the Octet rule. The only way that Hydrogen could be added is by breaking double bonds and stabilization (Resonance). And steric hindrance would be another key facet slowing the addition of an Iodine ion to the

1. INITIATION: Chlorine breaks down into free radicals that will then attack the methane molecules

On day 2, the experimentally determined rate law for this reaction was found to be:

There was a pattern with heat change. When 0.10 grams of CaCl2 was added, the temperature would increase. There seemed to be a negative correlation with how long the second reaction lasted, which would mean the reactions lasted for a shorter time for every 0.10 grams of CaCl2 was added. The color and smell remained constant throughout the whole experiment regardless of how much CaCl2 was added. For every 1 gram of CaCl2 added, the average time decreased by 18.2 seconds.

When we added the 1% silver nitrate to the alkyl halides in the first part of the experiment the first two test tubes, containing 2-bromo-2-methylpropane and 2-bromobutane, became cloudy almost immediately. The 2-bromo-2-methylpropane and 2-bromobutanes’ cloud was light green in color. The 1-bromobutane precipitated, though more slowly than the first two tubes, and its cloud was white. We also noticed that the 1-chlorobutane never seemed to become cloudy or precipitate. This is likely because chloride is a worse leaving group than bromide is (due to the chloride anion being a smaller ion, it can’t “handle” the negative charge as well as the larger bromide anion, so it doesn’t want to leave the carbon it’s sharing the electron with in 1-chlorobutane).

When reactions were carried out in the absence of a catalyst for long periods of time (180 min under solvent-free conditions), the yields of products were low (< 5 %) (Table 2, Entry 1). Better yields and shorter reaction times were obtained when the reaction was carried out in the presence of 0.05 g of the catalyst under solvent-free conditions (Table 2, Entry

Therefore, it can be seen using the collision theory that the more concentrated the reactants are, the more likely the molecules will collide and consequently speed up the reaction rate. This has been justified in the experimental results, when the more concentrated hydrochloric acid was, the faster the reaction rate. As shown in Experiment 1, where three different concentrations of hydrochloric acid were used. In Beaker 1, 0.5 M of hydrochloric acid was used, Beaker 2 was 1M, and in Beaker 3, 2M of hydrochloric acid was tested. It was shown in the experiment that the first beaker of 0.5M HCl took the longest to go cloudy, around 44 seconds. Beaker 2 had 1M of HCl and took 38 seconds, which was approximately 6 seconds faster than Beaker 1. In Beaker 3, 2M of HCl was added and it was the fastest of all three, taking 33 seconds, which was 11 seconds faster than Beaker 1, and 5 seconds quicker than Beaker 2. These results demonstrate that the concentration of the reactants does affect reaction rate as it was shown that an increase in the concentration of HCl meant that the reaction rate sped up, and vice

The melting point of a chemical is a physical property inherent to that substance. The chemical changes from a solid to a liquid state, but the composition remains the same. It can be used to determine the identity of an unknown substance. The purpose of this experiment was to discover the identity of an unknown chemical by determining its melting point.

Organic chemists use melting points to identify compounds and determine its purity. Two temperatures that need to be noted are the point at which the first drop of liquid appears from the substance and the point at which the entire mass of the solid substance turns to liquid. The range between these two points is the melting point. The melting point is used to determine the purity of a substance because if the substance is pure then its melting point will be higher. Also, if the substance is pure then its melting point will be narrower. The melting point will be lower if the substance is impure. Melting point can be used to identify an unknown compound by mixing it with a known substance with a known melting point. If it is the correct material

The hypothesis for this experiment stated that as concentration increased, the rate of reaction would increase as well. The experiment proved this hypothesis partially correct. The data supported the hypothesis since between 0.4 M and 1.6 M hydrochloric acid, the rate of reaction increased as

Melting point, a physical property, can be used to determine the identity as well as the purity of a compound. The purpose of this experiment was to utilize a DigiMelt melting point apparatus to determine the melting points of several crystalline substances. Pure substances have higher melting points and narrow melting point ranges compared to impure substances. Melting point range is determined by recording the temperature at which the substance begins to melt and the temperature at which the substance is fully melted. A compound can also be identified by using melting point; an unknown substance can be mixed with a known substance that has a known melting point and if the melting point is not the same as the known substance’s melting

The purpose of this experiment was to determine the melting point and the boiling point of various unknown solids and liquids supplied by the laboratory. In the process of exploring the most basic physical properties of the given samples, skills such as: proper determination of compound purity through different means and how to

Melting point of Tramadol hydrochloride- Paracetamol was determined by capillary method. The melting point of Tramadol hydrochloride was found to be in the range of 180 0C.The reported melting point is about 180-184 0C and of Paracetamol is 169 0C.