Kinetics of the Decomposition of Hydrogen Peroxide Lab Introduction: In this week’s lab experiment, the rate of decomposition of hydrogen peroxide forming oxygen gas will be observed and studied. Since the rate of a chemical reaction is dependent on two things; the concentrations of the reactants and the temperature at which the
Determination of a Rate Law Megan Gilleland 10.11.2012 Dr. Charles J. Horn Abstract: This two part experiment is designed to determine the rate law of the following reaction, 2I-(aq) + H2O2(aq) +
Classifying Chemical Reactions Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.
Conclusion: The objective of the experiment was to observe different reactions with different chemicals. The experiments emphasized on the chemical changes occurring in acids and bases as well as color changes and bubble formations. The experiments allowed for a better understanding of the undergoing chemical changes in mixtures. Some mixtures instantly changed colors while others were transparent or foggy. Some mixtures produced thick color that created solids called precipitates. Mixtures KI + Pb(NO3)2 and NaOH + AgNO3 both produce noticeable precipitates after a while. It was interesting to see the different acidic and base reactions like the fuchsia color formation in NaOH + phenolphthalein.
Procedure: Filled each test tube with substances provided and subjected them to various conditions. These conditions included, heat, cold water, hot water, acid and basic additions and tested on litmus paper. The reactions were observed and documented at each step.
The hypothesis that as (the first variable being tested), the concentration in the solution is changed and it becomes more dilute, this will result will be a slower rate of reaction. Therefore, it is also hypothesised that the addition of a catalyst will cause the rate of those reactions to speed up, was proven correct by the results of this experiment, in that the changing of the concentration and the addition of a catalyst changed the speed at which the reaction occurred. The results from both Part 1 and Part 2 conclusively showing that the have a direct effect on the rate at which the reaction occurs. In order to come to this conclusion, the data needs to be transformed into rate laws.
Abstract The free radical chlorination of 1-chlorobutane resulted in a mixture of at least 4 different possible products from the reaction. Gas chromatography-mass spectrometry helped in figuring out which of the products are most abundant in the sample product created as well as in discovering the ratio of relative reactivities of
6I-(aq) + BrO3-(aq) + 6H+(aq) → 3I2(aq) + Br-(aq) + 3H2O(l) The reaction rate for this is slow at room temperature. The definition of reaction rate is the rate of change in concentration of either reactants or products. It is dependent on the concentration of the reactants and on the temperature. In a rate law, a mathematical expression, the relationship between the reaction rate and the concentrations of reactants can be demonstrated. For example, the rate law for the rate of decrease in concentration of bromate ion would be:
Kalah Bailey October10th 2015 Chem 109 Pre-Lab 6 Title: Observations of Chemical Reactions. In this lab, students will recognize and record the chemical reaction results of seven different anions and one cation. This experiment also focuses on the reaction of salt solutions and what happens when two different solutions mix.
From the testing and results several major trends and relationships were discovered. The first observation, which supports the hypothesis, is the relationship between concentration of reactants and reaction rate. As concentration increased, the reaction rate also increased in direct proportion. This was shown by the results because when the concentrations doubled, from 0.1M and 0.125M to
They observed an increase in initial rate with increasing the concentration of substrate but after 40 minutes the degradation efficiency decreased with increasing initial concentration (figure7). A pseudo-first-order kinetic was assigned to the reaction and the initial rate of the reaction for different concentrations was measured. Using Langmuir rate model and the initial rates, rate constants in different pH values were calculated. Acidic pH (3.5) showed higher reaction rate due to favored interaction between positive surface of catalyst and oxygen atoms. pH 9.5 showed higher rate constant supposedly caused by substrate hydrolysis in basic solution
Each reaction would be carried out by mixing five different solutions four times separately and each reaction is consisted of KI solution, starch solution, Na2S2O3 solution, KNO3 solution and EDTA solution. The concentration of each solution varies because the first reaction include 25.0ml KI solution, 1.0ml starch solution, 1.0ml Na2S2O3 solution, 48.0ml KNO3, 1 drop EDTA solution and the total volume eqaul 75.0ml. The second reaction include 25.0 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3 solution 23.0 mL KNO3 solution 1 drop EDTA solution and total volume equal 50.0ml. The third reaction include 50.0 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3 solution 23.0 mL KNO3 solution 1 drop EDTA solution and the total volume equal 75.0 mL and the fouth reaction include 12.5 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3 solution 35.5 mL KNO3 solution 1 drop EDTA solution and total volume equal 50.0ml. After obtaining all of the solutions and seven different test tubes of 1.0ml Na2S2O3 solution which should be pour into the Erlenmeyer flask whenever the color of the solution changes. To calculate the reaction rate of each reaction the timer should start immediately when all of the solutions are mixed. Once all of the solutions have been mixed the students should observe as well as record the time of the reaction when the color change to dark blue and one of
DISCUSSION By analysing the results of The Landolt clock reaction, and the outcomes that occur due to change in concentration and the addition of a catalyst, the data did partially support the hypothesis. That by changing the concentrations of potassium iodate and sodium bisulphite the rate of the reaction will increase. The rate gradually increased per every 10 seconds on the NaHSO3 graph. Whereas compared to the KIO3 graph the rate was more efficient, the reaction was achieved within 5 seconds. However, the second hypothesis regarding the addition of a catalyst, displayed acceptable results. The catalyst increased the speed of the reaction within 10 seconds, which was slightly faster than the reaction times gained from the
The data supports the hypothesis that an exponential relationship will be found between the change in temperature and the reaction rate, and that the highest temperature will have the fastest rate of reaction. The data also supports the hypothesis that as the concentration of Potassium Iodine increases so will the reaction rate, and vice versa for an increase in Sodium Thiosulphate concentration. The hypothesis that the Iron (II) ions will affect the reaction rate, and that the optimal amount will be about 0.1M of catalyst was partially supported.
Purpose: The activation energy lab centralized on observing the effect that temperature has on the rate of the reaction 6I- (aq) + BrO3- (aq) + 6H+ (aq) 3I2 (aq) + Br- (aq) + 3H2O while also using calculations to determine the value of the rate constant and the activation energy at different temperatures. The activation energy of a reaction is defined as the minimum amount of energy required to make the transition from reactants to products. Given that the rate constant is proportionally constant for an experiment, it changes with temperature. By keeping the concentrations of the reactants constant, the effect of temperature on the rate was able to be determined.