We need to be able to find the limiting reagent and be able to go through the process of gravimetric stoichiometry. Hypothesis: The limiting reagent will be the strontium chloride due to the calculations and the copper (II) sulphate pentahydrate. My calculations also conclude that we should get 1.378 g of the precipitate of Strontium Sulphate. SrCl2 * 6H2O + CuSO4 *5H2O SrSO4 + CuCl2+ 11H2O I Mole 1 Mole 1 Mole 1 Mole 11 Mole 2g 2g ? Materials: • 2 Graduated Cylinders • Distilled Water • Stirring Rod • Balance • One 250ml Beaker • One Erlenmeyer Flask • Filter Paper • Copper (II) Sulphate Pentahydrate • Strontium Chloride Hexahydrate Procedure 1.
INTRODUCTION OF CHEMICAL REACTION A chemical reaction is a process in which one set of chemical substances (reactants) is converted into another (products). It involves making and breaking chemical bonds and the rearrangement of atoms. Chemical reactions are represented by balanced chemical equations, with chemical formulas symbolizing reactants and products. A chemical equation is a way to describe what goes on in a chemical reaction, the actual change in a material. Chemical equations are written with the symbols of materials to include elements, ionic or covalent compounds, aqueous solutions, ions, or particles.
Adjust the percent transmittance to 100% 4)our out the water in the cuvet, and fill with 2/3 of the reference solution. Read and record absorbance data. Read from lower concentration to higher concentration. 5)Continue to collect absorbance data for al reference and test solutions 6)Dispose of the contents of the cuvets. Data Tables #1 Reference Solutions for the Calibration Curve Sample [FeSCN2+] Absorbance Reference Solution #1 4x10-5 .2034 Reference Solution #2 6x10-5 .3028 Reference Solution #3 8x10-5 .3915 Reference Solution #4 1.0x10-4 .4908 Reference Solution #5 1.2x10-4 .5768 #2 Test Solutions Temperature - 21.9°C Sample [Fe3+] [SCN-] Absorbance Test Solution #6 1.0x10-3 2.0x10-4 .1002 Test
Chemical kinetics Date: 20th, Aug., 2010 Name: Huang Shiqi A0078026E Email address: sunnyqi0801@gmail.com Class No. : Fr1 Lab partner: Jerome Lime A0073046L Abstract: The stated objectives of the experiment were to determine the reaction orders and rate constant of a chemical reaction, using the method of initial reaction rates and to determine the activation energy from the temperature dependence of the reaction rate based on Arrhenius’ theory. The chemical reaction used was iodide-persulfate reaction. Based on the equation: R = k [I-]n[ S2O82-]m and Arrhenius equation, the orders, rate constant (k) and activation energy can be calculated. The orders of the reaction were 2(n=m=1), k was 0.004174 L mol-1s-1 and the activation energy was 82.577kJ/mol.
The paper discs were dipped in the samples given, one being a Yeast solution and the other a Catalase solution. After that, the discs were then immersed into the H2O2 solution. The oxygen produced from the enzyme reaction will form on the disc and cause it to float upwards to the surface of the H2O2 solution. Through these procedures we can investigate the effects of substrate concentration on the rate of reaction. We can manipulate the substrate concentration by varying the concentration of H2O2 taken during each trial of the experiment and measure the rate of reaction by measuring the time taken for the paper disc to float to the surface.
ABSTRACT: The purpose of this experiment was to determine the rate constants and ionic strengths of the series and to prove the Bronsted relation. In order to do so, known amounts of KI, Na2S2O3, KNO3, EDTA, starch and K2S2O8 were mixed up, and placed in the spectrophotometer until the %T reached 60%, and time was recorded. In the first part of the calculations, for flask 1, 2 and 3, the true reaction rate was calculated using the equation k = (1/∆t) x ([S2O32-]/[Iodine][S2O82-]). Which resulted in values of 2.8878765.66 x 10-3 s-1 , 3.159845 x 10-3 s-1, and 3.079703 x 10-3 s-1, these values are all similar to each other since they contain no electrolyte reacting with the persulfate solution. The apparent reaction rate was calculated using the equation, kapp= (1/∆t) x ([S2O32-]/[S2O82-]) which resulted in apparent rate constants of 5.66 x 10-5 s-1, 6.1958 x 10-5 s-1, 6.0356 x 10-5 s-1.
Nathan Bahn Beer’s Law Study Lab Introduction: In this lab, we used a spectrometer to observe the transmittance of light at a certain wave length. We experimented to see if the molarity of a solution changes the transmittance of light and the absorbance of that light by the solution. By observing the percent transmittance and the amount of light absorbed, we can calculate the amount of color absorbing components in the solution. Through this process is how we are able to discover the amount of copper in the solution. Experimental Procedure: 250 mL of the copper solution was made by creating 100 mL of the solution, reacting CuO with HNO3, and then diluting to the mark of 250 mL.
Chemical Kinetics: Iodine Clock Experiment Bautista, Lance Ruther E., Tornalejo, Norielle Marie B. Abstract: Is Iodine clock really a clock? In what way do we relate temperature with the rate of the reaction? How about the relationship between the concentration and rate of reaction? In this experiment, the effect of concentration and temperature on the rate of a chemical reaction will be studied. For this experiment, when the temperature increases, collision between the particles also increases.
Initial rates of solutions of the same consistency were determined by measuring the optical rotation angles at various temperatures. The data obtained was used to construct an Arrhenius plot and the activation energy for the reaction was determined. The values obtained through this experiment are as follows: α(0)=4.42 ± 0.06˚, α∞=-1.355 ± 0.001˚, k2cE0= (3.00 ± 1.15) x 10-4 (M/s), Km=1.1 ± 0.4 x 10-1 (M), and k2=(3.60 ± 1.38) x 10-4(s-1). INTRODUCTION In the study of chemical kinetics, the rates of enzyme catalyzed reactions are a significant area of interest as virtually all biochemical reactions are catalyzed by this class of proteins.1 For enzyme-catalyzed reactions, the basic mechanism as shown below in equations 1 and 2, was first proposed by Michaelis and Menten and then verified by a study of the kinetics of the inversion of sucrose.1 Eqn 1: E+S ES Eqn 2: ES E+P In this simple reaction mechanism an enzyme, E, converts a substrate, S, into products, P, through the initial formation of an enzyme substrate complex, ES. Using
Experiment 7 Additivity of Heats of Reaction: Hess’s Law Introduction This report discusses an experiment that combines equations for two reactions to obtain the equation for a third reaction, uses a calorimeter to measure the temperature change in each of three reactions, calculates the heat of reaction (∆H) for three reactions, and uses the results to confirm Hess’s law. This experiment will use a Styrofoam-cup calorimeter to measure the heat released by three reactions. These measurements of heat released will be used to confirm Hess’s law. Hess’s law states that the heat of reaction of the one reaction should be equal to the sum of the heats of reaction for the other two. In the case of this experiment one of the reactions performed will have the same amount of heat released as the other two reactions combined.