Looking back at the research question, the actual amount of reactant did not match the theoretical stoichiometric amounts according to the balanced equation, but the amount of catalyst matched the original value when uncertainty is taken into account. The percent yields for the reactants in the equation are very far from 100% yield. In the case of water, the percent yield came out to be meaning there were at least 2 times to 4 times more water than there should be. The percent yield of oxygen came out to be , around 2%, maybe higher considering uncertainty of what amount of oxygen there was suppose to be. The reaction was incomplete and had to be stopped because of time, which explains the very high percent yield of the water and the very low percent yield of oxygen. The yield of the catalyst though, came out to a perfect , which means that including uncertainty, there was as much MnO2 that came out of the reaction as was put in the reaction. This proves that catalysts do not get consumed in the reaction, with added evidence that even though the reaction was incomplete, the catalyst was not affected and therefore is not a part of the products or reactants and is not consumed. Based on uncertainty analysis, I have a very low degree of confidence in the results regarding the reactants mainly because of procedural uncertainty. I have a strong degree of confidence in the result regarding the catalyst because of the small uncertainty.
The method of the experiment resulted in a large degree of uncertainty in the results. There were two major sources of procedural uncertainty. The source that affected the data the most was due to the fact that because of time limitations, the reaction had to be cut short and stopped at around 10 minutes after the start of the reaction. As a result, the reaction was incomplete, leaving un-reacted products and reactants that weren’t produced yet and therefore any measurement of the reactants, oxygen and water, was skewed. The direct...
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