Experiment : Melting Point And Percent Yield Of Dimethyl Fumarate

The main objective of this experiment is to differentiate between a physical change and a chemical change.

The mixture was transferred to an ice bath to crystallize the product, after which the product was collected by vacuum filtration on a Hirsch funnel, washing the flask with small aliquots of cold xylene and pouring the solution over the crystals, allowing the vacuum to thoroughly dry the product. Additional drying was achieved by transferring the product to filter paper and pressing the crystals to remove any excess moisture. The product was then weighed and a melting point determined. A comparative TLC was run in Hexanes:Ethyl Acetate solvent against maleic anhydride to verify the purity of the

Calorimetry is the science of measuring the change in heat absorbed or released during a chemical reaction. The change in heat can tell us if the reaction is either exothermic - it released or heat into surroundings, or endothermic - it absorbed heat from surroundings. The device used to measure calorimetry is a calorimeter. A calorimeter can range from very expensive lab ones to coffee styrofoam cups but they are all tightly sealed in order to prevent heat from escaping.

The purpose of this lab is to test substances and to determine the physical and chemical properties of substances.

With a molecular weight of 180.2 grams/mole, this is equivalent to 0.00499 moles initially. 0.941 grams of the product, stilbene dibromide was collected upon completion of the experiment. With a molecular weight of 340.0 grams/mole, this amounted to 0.00277 moles of product. This gives a percent yield of 55.5%. The melting point of the product was found to be between 250C and

The product obtained had a melting point of approximately 107 °C and a weight of .324 grams. Some of the product would not dissolve in water and so was removed through vacuum filtration, which left .141 g not dissolved in solution. It took 13.2 mL of sodium hydroxide to turn the solution of the product dissolved in water pink. A molecular weight of 138.63 g/mol was calculated from the data. These results indicate that the product was 2-methylbenzoic acid, the Grignard reagent was 2-methylphenylmagnesium bromide, and the unknown bromide solution was 2-methylbromobenzene. Calculations showed that the limiting reagent of the Grignard preparation was magnesium and that the experiment had a 23.13 % yield.

Day 1. Michael was coming home for vacation from college. When he got home he found out that

Snow globes are made of clear glass, a transparent sphere with a scenic view and a plastic toy inside the globe. The globe must be shaken to actuate the snow so the white particles can fall gradually to reach the base. When the marble (object used for this experiment) falls, it experiences two external forces which are; the gravitational force and the aerodynamic (fluid resistance) drag of the marble, which affects the rate of the marble. As the marble is falling, the speed is increased due to the gravitational force, which is pulling the marble downwards to the base of the beaker until it reaches the terminal velocity, where both external forces are equal. However, there are factors that can affect the marble’s terminal velocity, such as

The boiling range of the 1-pentyl ethanoate distillate was approximately between 149-151°C. This was indicated by the formation of the distillate and when the mixture of the purified 1-pentyl ethanoate started to vigorously

Sugar in Coke Lab Report Sheet: Raghed Odeh 10/18/2017 Provide a brief statement of the purpose of this activity and explain the idea behind a calibration curve (this can be done before class and valuable insight can be gained by watching the “weblets” (online prelab lectures available in the course content of D2L). The purpose of this lab is to determine the amount of sugar (in grams) in a can of coke, learn how to make solutions quantitatively and learn how to make and use a calibration curve. A calibration curve is used to understand the instrumental response to an analyte and predict the concentration in an unknown sample. As long as a function is known, the curve can be made.

The purpose of this experiment is to identify an unknown substance by measuring the density and boiling point. I will be able to conclude which substance is my own from a list of known options stating what its real boiling point and density is.

The result was small white crystals, which were dry and had barely contained any moisture. The product was then dissolved in methylene chloride and dried with granular anhydrous sodium sulfate. The drying agent would have removed any water in the solution and presented a colorless solution. The solvent was evaporated and the product was collected; it had the appearance of small, white solids. Data Table 2 shows the results and calculations that were gathered after the completion of this experiment. A boiling point of the product was found to be 210℃. According to literature, the boiling of isoborneol should be 212℃. As a result, the product is most likely isoborneol. No errors had occurred during the course of the experiment, which is testified by the high yield of

The purpose for this experiment is to determine if different proteins denature, physically change, at the same temperature. By doing this, we can prove that not all proteins are made the same, and that they have different structures.

The beaker was slowly heated on a hot plate with low stirring until most of the stilbene was dissolved. 0.4 g of pyridinium tribromide was measured and added to the beaker after 5 minutes of heating. Small amounts of ethanol were used to clean the sides of the beaker. The beaker was heated for an additional 10 minutes on low temperature. An ice bath was prepared. The beaker was removed from the hot plate and left to cool to room temperature. Once at room temperature, the beaker was placed in the ice bath for 15 minutes. The solid product was collected through vacuum filtration and the product was weighed and a melting point was taken. Waste was disposed of in the correct waste bins and lab bench was cleaned

Overall, the experiment succeeded that the metals show the theoretical properties. Differences existed in the mathematical calculation of the actual length. These differences, however, it can be accounted for by experimental error; more over there are uncertainty on purity of the