1) Coronary artery disease occurs when fatty deposits called plaque build up inside the coronary arteries. The coronary arteries wrap around the heart and supply it with blood and oxygen. When plaque builds up, it narrows the arteries and reduces the amount of blood that gets to your heart. This can lead to serious problems, including heart attack. 2) Coronary artery disease is usually caused by a build-up of fatty deposits on the walls of the coronary arteries.
My hypothesis for the experiment was that the optimum temperature for catalase to function is 98.6o F because this is the optimum temperature for the human body. The optimum pH level for the catalase function is 7 because the human’s optimum pH is 7. Materials and Methods Forceps Test Tubes Raw Liver Hydrogen Peroxide Test Tube Rack Gloves Goggles Pipette Waste Beaker Beakers Hot Plate Ice Bath Thermometer The procedure that we used to do the normal catalase activity was that we first transferred 2 ml of hydrogen peroxide solution into a clean test tube. Next we took
The pipette was then filled with 25.0mL’s of acetic acid and then drained into a conical flask, to speed up the process both of the conical flasks were filled with 25.0mL of the acetic acid. 8. Three drops of phenolphthalein was then added to the flask with the acetic acid. 9. The conical flask was then positioned to just under the burettes dropper which had its stopcock opened to allow a medium drip rate and had the sheet of filter paper slipped under it so that the colour could be seen more earily.
The effectiveness of lipase on temperature Abstract Enzymes are biological catalyst that speeds up the rate of reaction. Different enzymes work best at different temperatures, which is also called an optimum temperature. Different enzymes also have different functions. Lipases are enzymes, needed to break down lipids (fats and oils) into the products - glycerol and fatty acids. They work best at room temperature around 36-40 C. Introduction For this experiment, I will be looking at how the change in temperature affects the rate of reaction.
Rates of Reaction - Marble Chips and HCl In this experiment, marble chips, or Calcium Carbonate (CaCO3), will be dropped into a flask containing Hydrochloric Acid (HCl). The reaction is: CaCO3(s) + 2HCl(l) --> CaCl2 + H2O(l) + CO2(g) The experiment will determine whether or not stirring quickens the reaction rate, which will be illustrated by the slope of the lines in the data graph. If heat and stirring is added to a reaction, then the gas will be released quicker. This is so because when two compounds interact, or collide, a reaction occurs. If the compounds are made to collide faster, by way of stirring, then theoretically the reaction as a whole will start faster and come to completion faster.
Given the results, we determined our experimental methods were effective in determining the content of calcium carbonate in the antacid sample. In the future, we will implement a centralized time keeping procedure to ensure increased efficacy of our experimental techniques. Introduction Heartburn condition, also known as pyrosis, non-cardiac chest pain or acid reflux, is a predominant ailment in our society. The condition causes painful burning sensation in the esophagus, and is usually associated with regurgitation of gastric acid. This is mainly due to the premature opening of the lower esophageal sphincter between the esophagus and the stomach.
When the solution is acidified during diazotization to form nitrous acid, the sulfanilic acid is precipitated out of solution as a finely divided solid, which is immediately diazotized. The finely divided diazonium salt is allowed to react immediately with dimethlaniline in the solution in which it was precipitated. Mechanism Diazotization: [pic] Diazo Coupling: Methyl orange is often used as an acid-base indicator. In solutions that are more basic than pH 4.4, methyl orange exists almost entirely as the yellow negative ion. In solutions that are more acidic than pH 3.2, it is protonated to form a red dipolar ion.
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.
Contents Page Experiment 1 Calibration of a 25-mL Pipette 1 Experiment 2 Volumetric Analysis 3 Experiment 3 Experiment 4 Experiment 5 Gravimetric Determination of Nickel Sodium Acid Salt of Heptaoxodiphosphoric Acid Synthesis and Stoichiometric Analysis of Hexaamminenickel(II) Chloride 5 6 9 Experiment 1: Calibration of a 25-mL Pipette Background The graduation mark on a pipette being usually made at 20°C (whereas room temperature is much higher than this), the volume of the pipette must be calibrated before any volumetric analysis is carried out. Otherwise, the error in the graduation mark may exceed the error allowed in a measurement. A pipette is designed to deliver only one fixed volume of a liquid and it is calibrated for this volume only. Accuracy to two decimal places in mL is generally possible. The pipette is calibrated by weighing distilled water in it at room temperature, and then calculating the volume from the weight of water in air.
The bomb is filled to about 20 atm of pressure with O2, sealed, and placed in a known amount of water. An electric current is passed through a wire to ignite the mixture. As the combustion takes place, the heat evolved raises the temperature of the calorimeter and its surrounding water, as measured by a thermometer. In order to prevent heat loss from the calorimeter system, some calorimeters are surrounded by a second water bath, whose temperature is continuously adjusted