Wittig reaction

An exothermic reaction is one in which there is a release of energy (usually heat) from the system (Ashworth & Little, 2001). In other words, the energy of the system decreases, and thus H is negative. Because heat is being transferred out of the system (i.e., the reaction requires no external energy source), exothermic reactions are self-sustaining (Ashworth & Little, 2001). Notable examples of exothermic reactions include combustion reactions, where oxygen (O2) reacts with another substance, usually

Discussion: - Describe what the results were After investigating the effect of temperature upon amylase reaction rate on starch, it was evident that the chemical reaction did occur. The beaker which was heated to 80 degrees Celsius changed to a brown colour after 5 minutes. The cold beaker (5 degrees) showed similar change, however the only beaker which didn’t change at all was the body temperature one. As seen in figure 1 and 2, each temperature were tested 3 times to gain reliability. Furthermore

makes more carbon dioxide in high temperature it is possible that the temperature would be so hot that it will end up destroying the yeast cells which will cause it to have less carbon dioxide. The reason for this is because of the rate of chemical reactions increasing along with increasing temperature. When one refers to the temperature of a system, it is described as the measure of the average kinetic energy of the particles in a sample of matter. Increases in the temperature of a system results from

magnesium strip in the test tube filled with liquid and time the reaction (time it takes for the strip to dissolve) with a stopwatch. Record the results in a table. 6. Put 8 ml of hydrochloric acid in a 10 ml measuring cylinder. 7. Put 2 ml of water in a 10 ml measuring cylinder 8. Once again, mix both substances in a test tube with a total volume of 10ml. 9. Drop a 1 cm magnesium strip in the test tube filled with liquid and time the reaction (time it takes for the strip to dissolve) with a stopwatch

Qualitative Observation of a Chemical Reaction Purpose: Carefully observe and interpret a chemical reaction. Apparatus: Equipment- 250mL beaker, 125mL Erlenmeyer flask, cardboard square, chemical scoop, metric ruler, lab countertop, rubber stoppers, safety goggles, lab apron Materials- candle ( 2cm diameter), matchbook, 2 toothpicks, Limewater solution, string, aluminum foil, Cobalt Chloride paper Procedure: Note appearance, odor, and feel of the unlighted candle. Heat the bottom of the candle

Substitution 5. Introduction In this experiment, a primary alcohol was converted into a primary bromoalkane using hydrobromic acid. The reaction was done under reflux and then distilled to obtain a product of higher purity. The degree of the alkyl halide obtained from the experiment was tested with silver nitrate and sodium iodide. An infrared (IR) spectra and the weight of the product were obtained for further analysis. The IR gave information on the present functional groups and product weight

temperatures, and with this experiment we hope to discover which temperatures are unideal for Catalase. The substrate is H2O2 which binds to the active site of the enzyme Catalase. The reaction in question is as written below: Hydrogen Peroxide + Catalase -> Water + Oxygen (Catalase is not consumed in the reaction) This question is important to understand because Catalase plays a vital role in the sustenance of cells and tissues

it happened. This demonstration is called the “whoosh bottle.” It is where you place a low-boiling alcohol such as methanol, ethanol, or isopropanol into a bottle, coat the entire bottle with the alcohol, and then use fire to create an combustion reaction

change of colour, the forming of a precipitate, the forming of gas bubbles, the production of heat or light, and if the change is difficult to reverse. In the chemical reactions lab, several chemical changes will occur. Participants must use this knowledge to decipher what change has occurred after the chemical

Chem 245-002 Yang 4/13/17 Short Paper #2: Oxidation of 4-nitrobenzyl alcohol To begin the oxidation reaction, first prepare the oxidant that will be used. To make the oxidant combine 390 mg of each of the following compounds: activated 4Ǻ molecular sieve, PCC, and anhydrous sodium acetate. This mixture should be grinded into a powder using a mortar and pestle. Once the oxidant is made the reaction can take place. Obtain a clean, dry 5mL conical vial with a spin vane. Add 1.17 g of the oxidant, 6