Yield Of Ester Lab Report

As only 4.3mL of ester was collected, there was a poor yield of ester in this experiment. This may have been because the amount of reactants used was too little (i.e. only 10mL of each), and thus, a greater yield of ester could not be produced. Moreover, the reflux time of 40 minutes may have been too short, and did not allow a long enough period for a sufficient volume of ester to be produced as they reactants were vapourised and condensed back into the pear-shaped flask to react. Additionally, as the esterification is an equilibrium reaction, 100% of the yield of ester could not be obtained. This is because, once the reaction reached equilibrium, the concentrations of all species in the reaction including the reactants and products remained

In improving the yield of the ester, the amount of reactants used could be increased, and as esterification is an equilibrium reaction, by Le Châtelier’s Principle, this will drive the equilibrium position to the right, thereby increasing the yield of ester. Additionally, water, another product of this reaction, can be removed as it is being formed to also, by Le Châtelier’s Principle, drive the equilibrium position to the right, again, increasing the yield of ester. This removal of water can be accomplished by adding more sulphuric acid, which is a dehydrating agent that has a strong affinity for water, thus absorbing it, and shifting the equilibrium position to the right. Moreover, the mixture can be refluxed for a longer period of time so that more of the reactants have the opportunity to be converted into ester. This modification would only be useful assuming the reaction did not reach equilibrium in the already conducted experiment. Furthermore, when discarding the aqueous layers and sodium carbonate layer from the separating funnel, experimenters could be more careful in making sure that part of the ester layer is not also lost in the

These include wearing lab coats so that any spillages, especially those of chemicals such as sulphuric acid, will not allow for contact with the skin to occur. As sulphuric acid is corrosive, it can cause severe burns and tissue damage when in contact with the skin or mucous membranes. Likewise, participants should ensure to wear protective glasses at all times to prevent any splashes of chemicals to reach the eye, and therefore, cause irritation or burns. If contact with any chemicals is experienced, an adult should be notified so that the appropriate treatment, such as washing the affected area with cold water or applying an ice pack can be undertaken. In more severe cases, medical aid should be considered. Moreover, as the Bunsen burner will often be used to heat the mixtures, participants should be careful when handling the heated glassware, waiting for them to cool down before touching them to prevent burns. Again, if any burns are experienced, a supervisor should be advised, and cold water or an ice pack should be applied to the affected area to relieve the burn or stop any swelling. Moreover, participants should be careful in the general handling of the glassware, ensuring that they are not placed near the edges of benches, but rather, near the back towards the wall. This is because, if the glassware were to fall, breakages would occur, increasing the risk of cuts occurring.