Kinetics Lab

793 WordsMar 16, 20114 Pages
¬¬¬¬¬¬04/28/2010 Monday & Wednesday 7:40-10:30 Experiment #2 – Kinetics of the Decomposition of Hydrogen Peroxide Introduction: Chemical reactions are dependent upon two factors: temperature and concentrations of substance. We can monitor the rate at which a chemical decomposes or the rate at which a chemical substance appears. In this experiment we will be measuring the rate of decomposition of hydrogen dioxide with the following reaction: 2 H202 (aq) 4 2 H20 (l) + 02 (g) We can trap the oxygen gas created into a container thus showing the extent of the reaction and this will show the rate in which oxygen is created and how the rate will change when we use different initial concentrations. We do use a catalyst in this reaction to…show more content…
It had a lot to do with the time and the amount of oxygen evolved. When holding the leveling bulb it seemed that the longer I had to hold it level the harder it became to be as accurate. I would find my arm getting tired and the bulb varying, which would also effect the times that we recorded. Another thing that could have affected our results was not putting the stopper on the Erlenmeyer flask fast enough, fumes from the formation of oxygen could have escaped before we got the stopper on, causing error in the amount and time in which the oxygen was evolved. Post Lab Questions: 1. 2. 3.
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