Record the initial temperature of the liquid in the calorimeter. Watch the thermometer until maximum temperature is achieved. Weigh out 2.0g of NaOH pellets. Record the temperature of the distilled water in the calorimeter until the temperature is constant then add all of the pellets at once. Gently stir the pellets until the acid is dissolved by shaking the the apparatus.
The initial volume of the buret was recored. The stopcock was opened and NaOH solution was added to the HCl solution. The Erlenmeyer flask was then gently twirled. This process was repeated until the HCl turned a very faint shade of
The graduated cylinder will collect the distillate. Make sure to leave area between the end of the distillation take-off and the cylinder so that you can see the drops of distillate leave the distillation apparatus. All experiments will be done using the Celsius temperature scale. Notice that the temperature displays in the neck of the round bottom flask. Step 2.
Experiment 14: Iodine Clock reaction Summary of principles: In this lab we will learn to measure the rate of a chemical reaction between persulfate ion and iodide ion. The order of the action will need to be determined in the order of the persulfate ion to the iodide ion. The method we will use is the Initial rate method. The activation of the reaction will be determined from the temperature dependence rates of the reaction. The lesson of the lab is to teach us about Chemical kinetics, speeds and arrangements of molecules in a reaction during the process it goes from reactants to products.
Chemistry 3/19/13 Calorimetry Lab Report Purpose: Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical purposes. The purpose of this lab was to use calorimetry to find how much heat is absorbed or released when NaCl is dissolved in water. In this case, we will find the heat coming out of the system, in a chemical process. Hypothesis: Once the sodium chloride is put into the water, the temperature of the water will rise. Procedure: 1.
Sodium Hydroxide + Hydrochloric Acid Sodium Chloride + Water NaOH(aq) + HClaq → NaCl(aq) + H2O(l) Variables Independent The independent variable of the experiment was the amount of sodium hydroxide that we added to the acid. To keep the variable controlled we would measure 1 ml of the sodium hydroxide and pouring that to the hydrochloric acid. Dependent The dependent variables of the experiment were the temperature and the pH number of the mixture. To control the pH and temperature use the electronic probe and data logger. Controlled The controlled variables of the experiment were: A.
Now to find this we would also have to look at the heating curve of the experiment. Also we have to look for when and how the physical change from a solid to a liquid (melting) happens to the Lauric Acid. * A heating curve is when you supply heat to an isolated material over a certain amount of time. To see the heating curve you must graph to noticeable see the rise and stabilization of the heat within the material. Also to further example this lab, Phase Change is when one state of matter changes to another state of matter through either endothermic or exothermic change.
A burette with the standardized NaOH solution is filled. The strength is recorded of the solution which it is marked on the dispensing bottle. Volume of the standardized base to neutralize the HOAc in the beaker is calculated. The electrodes are used to calibrate. The buffer is removed and rinsed with the electrodes with distilled water.
57 THE IODINATION OF ACETONE Part One: Determining the Rate for a Chemical Reaction The rate of a chemical reaction depends on several factors: the nature of the reaction, the concentrations of the reactants, the temperature, and the presence of a possible catalyst. In this experiment we will first determine the rate law for a reaction by changing some of the above variables and measuring the rate of the reaction. During Part Two, we will explore the relation between the rate constant and temperature to discover the activation energy for this reaction. In this experiment we will study the kinetics of the reaction between iodine and acetone: O C H3C CH3 + I2(aq) H3C H+ O C CH2I + HI(aq) The rate of this reaction is found to depend on the concentration of the hydrogen ion (acid, HCl) as well as the concentrations of the reactants (acetone and iodine). The rate law for this reaction is rate = k[acetone]m[H+]n[I2]p where k is the rate constant for the reaction and m, n, and p are the orders of the reaction with respect to acetone, hydrogen ions (acid), and iodine, respectively.
Experiment 1: The Reduction of Methyl Oleate Purpose: This experiment was carried out to gain a better understanding of the reduction of methyl oleate to methyl stearate. This experiment was carried out to determine whether or not the Markovnikov product or anti-Markovnikov product is prominent in this reaction. The final product will be analyzed by , and HMNR. Reaction: Summary of Procedure: The first step in this experiment was to flame dry the glass surfaces in the apparatus being used. Once dry, 2.2 mL of styrene were added to the round bottom flask, and an ice bath and mechanical stirrer were placed under the reaction vessel.