Melting Points Lab Abstract: One of the physical properties most relied upon for compound identification is a compound’s melting point. This experiment gives the student an opportunity to explore how compounds can be identified with this physical indicator. The experiment uses two compounds, tetracosane (C24H50) and 1-tetradecanol (C14H30O). The experiment confirms through melting points that the compound with more carbons and no branches (C24H50) has a higher melting point than 1-tetradecanol. Hypothesis: Using melting points can help determine the difference in total carbon atoms and branches between two or more compounds.
Also, the more stable the free radical that is left behind, the weaker its C-H bond strength will be. The difference between the bromine and chlorine product ratios can be partially explained by the Hammond postulate, which states that species with similar energy levels also have more similar structures and react more quickly and less selectively. In the experiment, five different hydrocarbons were tested to measure the rate of reaction with the addition of bromine. Two trials were done, one with the test tubes containing the hydrocarbons and added bromine sitting directly under a lamp, and another with the test tubes in a closed, dark space. Both trials contained a
Discussion and Conclusion In this experiment, the bromination of an alkene will be observed and a mechanism to account for the occurrence distribution of the products will be determined. In the first part of the experiment the 0.9 grams of E-stilbene will be put in a flask with 10ml of dichloromethane and then stirred to affect dissolution of the E-stilbene, since dichloromethane is a nonpolar solvent which can dissolve the nonpolar alkene. After the E-stilbene has been dissolved, 5ml of bromine in dichloromethane will be added, which will be stirred for thirty minutes until the solution is white, to ensure that the reaction has gone to completion. Bromine in dichloromethane is used because dichloromethane works as a good solvent for bromination reactions, due to the fact that it doesn’t react with bromine or most other organic molecules. The reddish color of bromine is discharged upon addition to an alkene as the bromine reacts, making this reaction a useful qualitative test for unsaturation when the reaction has gone to completion.
Observing Changes – Materials & Procedures Materials Water Copper (II) sulphate (Powder) Copper (II) sulphate solution Iron nail Sodium carbonate Hydrochloric acid Magnesium ribbon Flame (candle) Sugar Aluminum foil Test tubes Test tube rack Tongs Medicine dropper Spoons Beakers Safety goggles Scoopulas Procedures Water and Copper (II) Sulphate Procedure 1. Add a small amount of solid copper (II) sulphate to a test tube with a scoopula. Record the physical properties. 2. Write a hypothesis on what you think will happen when water is added.
5a. Place a small amount (the size of an aspirin tablet) of copper II sulfate pentahydrate in a clean dry test tube and record your observations. Using your test tube holder, tilt the test tube and gently heat the contents for 4-5 minutes, while recording your observations. Make sure to observe the upper end of the test tube while heating. Allow the test tube to cool and record your observations.
This was done by taking small amounts of the unknown acid. It was then placed into capillary tubes and inserted into the Bibby Sterilin Device. Starting with a high plateau to find a quick melting point and then proceeding to find an actual melting point. The next experiment that aided in finding more characterizations of unknown #2651145-PLF13 was equivalent weight. In order to find the equivalent weight a titration of the unknown acid had to be conducted.
Add a quarter spatula of copper (II) oxide and warm the solution gently to the 4th test tube and record observations. 7. To the 5th test tube, add 3cm3 of ethanol a couple of drops of conc, sulphuric acid and warm gently. Pour the resulting mixture into 30cm3 of sodium carbonate solution to remove excess acid and smell and record observations. Experiment 2 Time | Observations | 5 minutes | Bubbled like sugar | Once salt water was added | Turned soapy white and thick | Equation: METHOD 1) Put 2 cm3 of castor oil into a 250 cm3 beaker and add 10 cm3 of 5mol.dm-3 sodium hydroxide from a measuring cylinder.
Lab 2: If we heat sand then conduction will occur. III. Materials Lab 1: * 500mL Beaker * Water * Hot Plate * 2 Thermometers * Food coloring * Stopwatch * Oven mitt Lab 2: * 500 Ml beaker * Water * Hot Plate * 2 Thermometers * Beaker of sand – about 150-200 mL * Stopwatch * Oven mitt IV. Procedure Lab 1 1. Gather all materials 2.
NaNO2 (.0217 mol) was added to the solution and was allowed to react for five minutes. 6M HCl was added slowly to the solution, and then allowed to cool for one hour in an ice bath. The reaction was vacuum filtered to a orange color, and washed with water, ethanol, and ether. The product was allowed to dry for five minutes on the funnel. The resulting product was [Co(NH3)5ONO]Cl2 based on the collected data and yield was 1.215g (.00465 mol, 77.19%) Summary of Physical Properties: [Co(NH3)5Cl]Cl2: Bp 278 °C (lit1 = >150°C) IR in cm-1: 3255 (s, N-H
Purpose of the Experiment: To produce diphenylmethanol from the reduction of benzophenone by using sodium borohydride as a reducing agent. To check purity of a product by using thin layer chromatography (TLC) and by performing a melting point. Introduction: The key step in the reduction of a carbonyl compound by either lithium aluminium hydride or sodium borohydride is the transfer of a hydride ion from the metal to the carbonyl carbon. In this transfer the hydride ion acts as nucleophile. The mechanism for the reduction of a ketone by sodium borohydride: (1) Method (Based on Chemistry Laboratory Manual): 1.