There are two types of calorimeters which are usually used.
Explain how you determined the order of the reaction in H2O2 and KI. The rate determining step, or slow step, must be step 1. Our rate law expression was determined experimentally to have an order of 1 for both hydrogen peroxide and iodine. Because the coefficients of both reactants in step 1 are one, the order of the proposed rate law of this mechanism would match the order of our determined experimental rate law if the first step was the rate-determining slow step.
I determined the order of the reaction for hydrogen peroxide and KI by first writing a general rate law, where the order of both reactants was unknown.
I then divided the initial rate laws for Parts I and II, which canceled out the hydrogen peroxide as the concentration of hydrogen peroxide did not change in these parts.
I was left with the concentration of iodine ion raised to an unknown power, and taking the log of this expression I was able to find the order for potassium iodide, which turned out to be 1. I then divided Parts I and III and took the log of that expression to find the order of hydrogen peroxide, which was also 1.
The reaction that occurred during this lab was the decomposition of hydrogen peroxide catalyzed with the presence of potassium iodide. However, this was not the exact reaction that took place.
We added KI to the hydrogen peroxide because KI is a known catalyst and it would speed up the reaction. Catalysts are defined by being substances that increase or decrease the rate of a chemical reaction without being consumed in the process.
If the proposed mechanism for the reaction between H2O2 and I— is correct, then the iodine ion perfectly fits the definition of a chemical catalyst. Therefore, the iodine added to the solution is never consumed; it never interferes with the reaction. The decomposition of hydrogen peroxide is spontaneous; it would occur no matter what over a period of time.
Adding iodine, however, considerably speeds up the reaction. Catalysts are incredibly useful and sometimes vital in chemistry because they are able to significantly change the rate of the reaction without interacting with the reaction itself.
One way we can measure the change in the rate of the reaction is by using rate laws. Rate laws are able to quantify the rate at which a reaction occurs; they are the basis of studying the kinetics of chemistry.
The degree of the coefficient tells us the order of the reactant for that particular rate law. This order signifies how much that reactant affects the rate of the reaction.
For example, if the order of the above reaction for A was 2 and the order for B was 1, the reactant A would affect the rate more than the reactant B.
We determined experimentally that the order for both H2O2 and I— was 1. This means that the concentration of both reactants affect the rate of the reaction equally. This follows in the chemistry of catalysts, as if the concentration of the catalyst increases, there would be more catalysts to speed up the reaction and the rate would increase.
Our determined rate law was. We found this through comparing several different variations of the catalyzed decomposition of hydrogen peroxide. In Part I, we established the basic parameters that we would use a 0. We then saw how changing the molarity for both reactants affected the initial rate.
The initial rate was determined to be the slope of the graph of pressure vs.1) Calculate the rate constant and write the rate law expression for the catalyzed decomposition of hydrogen peroxide.
Explain how you determined the order of the reaction in H 2 O 2 and KI. Hydrogen Peroxide Decomposition Reaction Kinetics Purpose: In this experiment, you will determine the rate law and activation energy for the iodide-catalyzed decomposition of hydrogen peroxide.
Overview: The decomposition of hydrogen peroxide is catalyzed by iodide according to the following reaction: 2H2O2 (aq) [pic] 2H2O (l) + O2 (g) The speed of the reaction is determined from the reactants being .
As this investigation investigates the effect of concentration of catalase on the rate of decomposition of hydrogen peroxide, the temperature, pH and concentration of hydrogen peroxide are kept constant throughout the experiment.
Abstraction: This lab was designed to detect the decomposition of H peroxide into it O and H2O. The equation for this reaction is H H2O + +1/2O2 therefore by mensurating volume and force per unit area of O2 generated the sum of O2 generated can be calculated which in bend can be utilized to find.
Decomposition of Hydrogen Peroxide Essay. A+. Pages:4 Words This is just a sample. To get a unique essay. This lab was designed to observe the decomposition of hydrogen peroxide into it oxygen and water. The equation for this reaction is H H2O + +1/2O2 thus by measuring volume and pressure of O2 generated the amount of O2 generated.
The decomposition of Hydrogen peroxide looks like this: 2H2 O2 Catalase 2H2O+02 Prediction I think that the higher the concentration of Hydrogen Peroxide, the more bubbles will come out. This is because there will be less Hydrogen Peroxide in the beaker so there will be less to decompose.