Decomposition of H2O2
Nicholas Acevedo
Chem 216 Lab T/Th 8-10:50
Mr. Torres
January 31, 2013
Experiment 2
Kinetics of H2O2 Decomposition
Introduction
When measuring the rate of a reaction one can measure the rate at which one of the product appears or the rate at which the reactants disappear. The actual rate of a chemical reaction however is dependent on two things; the temperature the actual experiment is performed at, and the concentration pertaining to the reactants. The rate of a reaction more often than not depends on the concentration of one or all the reactants being used in the chemical reaction. This relationship that shows dependence can be expressed mathematically by the rate law, this can not be determined by just looking at a chemical equation it has to be determined experimentally as done in this experiment. In this experiment we will be looking at the rate of the decomposition of hydrogen peroxide, which yields liquid water and gaseous oxygen.
2H2O2 (aq) 2 H2O(l) + O2(g)
In this chemical reaction we will be examining the rate at which the product appears, in this case the rate at which oxygen gas is produced. This experiment will be performed more then once at different concentration levels to see how the rate of a reaction changes as the one changes the concentration levels. For this experiment we will also be using a catalyst to speed up the production of oxygen gas. The catalyst being used will be iodide ions, which will be introduced into the actual reaction through a mixture of potassium iodide, KI.
Once all the reactions are complete the rate will be found by using the rate law, which shows the dependence of the rate of the reaction of both the iodine and the hydrogen peroxide.
Procedure
For this experiment we had to work in pairs. First we assembled an apparatus with a flask, buret and a leveling bulb all attached with plastic tubing. Fill the plastic tubing with room temperature water through the leveling bulb until both are full.
Chem 216 Lab T/Th 8-10:50
Mr. Torres
January 31, 2013
Experiment 2
Kinetics of H2O2 Decomposition
Introduction
When measuring the rate of a reaction one can measure the rate at which one of the product appears or the rate at which the reactants disappear. The actual rate of a chemical reaction however is dependent on two things; the temperature the actual experiment is performed at, and the concentration pertaining to the reactants. The rate of a reaction more often than not depends on the concentration of one or all the reactants being used in the chemical reaction. This relationship that shows dependence can be expressed mathematically by the rate law, this can not be determined by just looking at a chemical equation it has to be determined experimentally as done in this experiment. In this experiment we will be looking at the rate of the decomposition of hydrogen peroxide, which yields liquid water and gaseous oxygen.
2H2O2 (aq) 2 H2O(l) + O2(g)
In this chemical reaction we will be examining the rate at which the product appears, in this case the rate at which oxygen gas is produced. This experiment will be performed more then once at different concentration levels to see how the rate of a reaction changes as the one changes the concentration levels. For this experiment we will also be using a catalyst to speed up the production of oxygen gas. The catalyst being used will be iodide ions, which will be introduced into the actual reaction through a mixture of potassium iodide, KI.
Once all the reactions are complete the rate will be found by using the rate law, which shows the dependence of the rate of the reaction of both the iodine and the hydrogen peroxide.
Procedure
For this experiment we had to work in pairs. First we assembled an apparatus with a flask, buret and a leveling bulb all attached with plastic tubing. Fill the plastic tubing with room temperature water through the leveling bulb until both are full.