This is because hydrogen bonds to the water molecules are formed. Acetaldehyde (ethanal, CH3CHO) and acetone are miscible with water in all proportions. II. Chemical Properties (see Bettelheim, chapter 17.4) Aldehydes are easily oxidized a fact due to the presence of the hydrogen attached to the carbonyl group (this is not present in ketones, which are less easily oxidized). Oxidation of aldehydes yields carboxylic acids.
Which of the 2 reactants is the limiting reagent C. Calculate the mass of urea formed D. How much excess reagent is left at the end of the reaction E. If the actual yield of urea formed was 980g what is its yield % a. Ans. 2NH3 + CO2 ( (NH2)2CO + H2O (17) (44) (60) 637.2 1142 980 b. HN3 c. 1124g d. 318g of CO2 e. 87.2% 1b .Iron is reduced from a reaction between aluminium and iron (III) oxide at a temperature of 3000°C. In this reaction 124g of Al and 601g of iron (III) oxide are reacted. A. Write a balance equation for the above reaction B.
* Let the crystals dry for one week, record the weight and take a sample and put into a glass capillary tube to obtain a melting point using the Melt-Temp machine. * Since volatile inflammable substances (ether, ethanol) and heat are used in this procedure, be very careful while conducting this experiment. Name | Structure | Molar Mass | Trimyristin | | 723.16 g mol−1 | Weight before recrystallization | Weight after recrystallization | % Recovered | Literature Mp | Experimental Mp | % Error | 2.0grams | 0.09 grams
Synthesizing Cyclohexene by Dehydrating Cyclohexanol Abstract 12.0mL of 85% phosphoric acid, 10.0mL of cyclohexanol and heat were used to perform an alcohol dehydration reaction and produce 5.85g of cyclohexene. The percent yield was found to be 74.84% after being washed with 10% sodium carbonate and dried with anhydrous Na2SO4. IR was used, along with a bromine test to confirm the identity of the newly formed cyclohexene. Introduction In organic chemistry, many different functional groups exist that have tendencies to react with each other in specific ways. Four main types of reactions relevant to this experiment are uni/di-molecular nucleophilic substitution (SN1 and SN2) and uni/di-molecular elimination (E1 and E2).
Make sure you graph along the rigid side because fingerprints on the clear sides can mess up the readings. You then pipet the amounts of material listed in Table 1 of your lab manual, then shake the mixes thoroughly. Turn on you spectrophotometer and set the wavelength dial 540 nm. Allow the instrument to warm up for ten minutes. Then prepare the unknown sample by pipetting 1 ml of the unknown solution into the cuvette and mix with 1 ml of dilute ferric nitrate.
Recrystallization of the Benzoic Acid Antonio Roki CHE 311L: Organic Chemistry I Section #2 September 14, 2012 Recrystallization of the Benzoic Acid Summary: The purpose of this experiment was to determine if the process of the Recrystallization is the good method of purification of the solid substance based on its different solubility values. This experiment conducted the purification of the Benzoic acid. The melting point range of the impure Benzoic acid was determined to be 86- 108 °C. Melting point was measured one more time after the process of the purification and was determined to be 111-117 °C. The melting point ranges of the impure and pure benzoic acid seemed reasonable.
OBJECTIVES In this experiment, you will • • • • Determine the freezing temperature of the pure solvent, lauric acid. Determine the freezing temperature of a mixture of lauric acid and benzoic acid. Calculate the freezing point depression of the mixture. Calculate the molecular weight of benzoic acid. Figure 1 MATERIALS Data Collection Mechanism Temperature Probe ring stand 400 mL beaker Tissue or paper towels lauric acid, CH3(CH2)10COOH lauric acid-benzoic acid mixture hot water bath utility clamp two 18 × 150 mm test tubes (if pre-made samples are not provided by your teacher) 1 “The Computer-Based Laboratory”, Journal of Chemical Education: Software, 1988, Vol.1A, No.
Slowly added the nitrating agent to the mixture of swirling methyl benzoate and sulfuric acid, adding the nitrating agent, drop by drop over a span of fifteen minutes, all while making sure the solution stayed submerged in the cold water bath. Finally, the solution rested in a water bath for fifteen minutes. The addition of ice was added to the reaction mixture and swirled around until all the ice was melted.
b) Add 3 drops of silver nitrate solution c) Note any color changes occurring d) Write a net ionic equation for any reactions that produces a precipitate e) Add a few drops of nitric acid to the test tube to acidify the solution. f) Mix well and note what happens to the precipitate. 4) In the third test tube: a) First add 1ml of bleach to a graduated cylinder adding 5mL of tap water and 6 drops HCL; Label an empty pipet and collect the solution into it. b) Br and I add 10 drops of the test solution to add 2 to 3 drops of the organic reagent and several drops of the chlorine water. Shaking the solution well, allow the lower layer to settle Note the color of the layer.
Name: ID number: 10346597 Experimental Title: Semi-Microscale Friedel-Crafts Reaction Members of Group: Date: Title: Preparation of 2-(4-Methylbenzoyl) benzoic acid from toluene. Introduction: The purpose of this experiment is to synthesis 2-(4-Methylbenzoyl) benzoic acid from toluene. Reagent Table: Reagents RMM (g/mol) Amount used (g) Phthalic Anhydride 166.14 1.0075 Toluene (sodium-dried) 92.14 5ml+6.5ml Aluminium Chloride 133.34 2.3 Hydrochloric Acid 36.46 3 ml Sodium Carbonate 105.9884 6.5 ml Light Petroleum Ether n/a 7.5 ml 2-(4-Methylbenzoyl) benzoic acid 240.25 Product Procedure The procedure followed was from Lab Manual CS262 page 48. The procedure was followed exactly; however one change to the procedure was made during the course of the experiment. A great deal of the crude product remained in the flask after its collection.