This raises the boiling point. After my apparatus was setup and distillation was begun water had condensates on the top of the fractionating column. This is to be noted since it can slightly affect the boiling point. As the distillation proceeded it was found that my distillation was occurring fairly slowly compared to other students. This issue was resolved with the addition of tin foil around the fractionating column and
Favourable Reaction Conditions One can use Le Châtelier's principle to explain the most favourable reaction conditions for the production of nitrogen (II) oxide. By decreasing the pressure, temperature or by adding/removing different components of the reaction, one could manipulate the equilibrium creating the most favourable reaction conditions. By decreasing the pressure the equilibrium will shift by producing more molecules in order to increase the pressure of the reaction again. The equilibrium will move in such a way that the pressure increases again. Due to the fact that the ratio of the molecules is 9:10 in the reaction, by decreasing the pressure the position of equilibrium will move towards the right-hand side of the reaction.
The experimental procedure followed is ideal for production of an abundant, but relatively impure sample of Aspirin. This outcome would be favorable with the hopes of using the produced sample in further experiments, rather than for commercial use. Introduction: The purpose of this lab was not only an introduction to the techniques for organic synthesis, but to apply stoichiometric techniques to calculate theoretical yield. Throughout the lab, the main process and procedure that was followed was Organic Synthesis, which allowed for the synthesis of aspirin to the greatest yield possible. In this case, the molecule that was synthesized was Acetylsalicylic acid, better known as Aspirin.
This is called the shaking and venting procedure. This procedure allows the benzoic acid (benzoic is the solute) to establish an equilibrium between the two layers the organic layer and the aqueous layer. Benzoic acid, although it has dissolve in water, is not very soluble in water (it will only dissolve in water at elevated temperature). However, benzoic acid is more soluble in methylene chloride. That is why once you add the benzoic acid aqueous solution and the CH2Cl2 in the separatory funnel the benzoic acid moves from the aqueous layer into the methylene chloride organic layer.
Catalysts operate by decreasing the value of the activation energy for the reaction. [1] The iodide ions lower the activation energy, making it easier for the reactants to convert to the products and vice versa, hence speeding up the reaction. We use an adaptation of the Arrhenius equation ln k’ = -Ea/RT + ln A . where k’ is the rate constant, Ea is the activation energy, R is the universal gas constant and T is temperature. [2] to determine the Activation Energy.
It is the one that we used in our experiment. Catalase will only work with Hydrogen Peroxide. It speeds up the breakdown of this toxic chemical into water and oxygen (2H202 (l) --->2H2O2 (l) +O2 (g)). Catalase is important because it breaks down Hydrogen Peroxide. Hydrogen Peroxide at high concentrations can be lethal.
If the solution of water and caffeine is mixed with the solvent dichloromethane, the caffeine is transferred to the dichloromethane. This results from the fact that caffeine is much more soluble in dichloromethane than water. Water and dichloromethane are not soluble in each other. The volatile dichloromethane can easily be vaporized off from the dichloromethane/caffeinesolution leaving fairly pure solid caffeine. In the process the solubilities of cellulose, tannins, and of chlorophyll will be considered.
The method to separate substances based on differences in their boiling temperature (volatile) is distillation. Many essential oils are separated from plant materials by steam distillation. The peel of oranges is boiled in water and the oil produced (limonene) distilled in steam at a temperature just below 100 °C, well below its normal boiling point. The immiscible oil can then be separated. Direct extraction by heating would result in decomposition whereas steam distillation does not destroy the chemicals involved.
Tannins, which are organic compounds that can bind to alkaloids such as caffeine, are going to be taken out of the tea water using sodium carbonate. The sodium carbonate is a base, which will convert the acidic tannins into sodium salts that are highly soluble in water. Isolating the caffeine will continue once methylene chloride is added to the remaining tea solution, which increases the solubility of the caffeine. Methylene chloride can be evaporated quickly leaving the caffeine to be purified by sublimation. Materials and Methods: The tea solution was obtained when a tea bag was placed in boiling water and its liquid mix was carefully squeezed into a beaker; and eventually placed into a test tube.
Similarly when the Calcium Carbonate (CaCO3) is broken down into powder the rate of reaction will increase. Because smaller pieces of the same mass of solid have a greater surface area compared to larger pieces of the solid. With this in mind when the Calcium Carbonate (CaCO3) is in solid form, the reaction rate will decrease. Procedure 1. Wear safety goggles 2.