Ethanol Oxidation Lab Report

Behavioral research on primates for medicinal purposes can result in unnecessary pain and suffering to the animals and doesn’t often ensure similar impacts in humans, is unnecessarily rehashed once the experimental results have been verified.The “Kinetics of Ethanol Oxidation” laboratory experiment utilized Beer’s law and spectroscopy to monitor concentration and the rate of ethanol oxidation through the LoggerPro System. This data then helped determine the kinetic rate constant, k, and the order of the reaction. First, the wavelength of maximum absorbance was determined using the LoggerPro interface and a Vernier colorimeter. Beer’s law was then used to determine the molar absorptivity. Finally, a kinetic study of ethanol oxidation was completed through the kinetic run on the LoggerPro interface. Chemical kinetics is the study of chemical reactions in relation to reaction rates. Kinetics is the study of motion. Molecules or atoms of reactants must collide with each other in chemical reactions.The molecules must have sufficient energy, or enough activation energy, to initiate the reaction. In some cases, the orientation of the molecules
They have more energy. When you lower the temperature, the molecules are slower and collide less. That temperature drop lowers the rate of the reaction.If there is more of a substance in a system, there is a greater chance that molecules will collide and speed up the rate of the reaction. If there is less of something, there will be fewer collisions and the reaction will probably happen at a slower speed. Pressure affects the rate of reaction, especially when you look at gases. When you increase the pressure, the molecules have less space in which they can move. That greater density of molecules increases the number of collisions. When you decrease the pressure, molecules don't collide with each other as often and the rate of reaction