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Unformatted text preview: molecules with sufficient energy to react will also increase. In Part 3, we let the decomposition of hydrogen peroxide (H 2 O 2 ) go to completion, measuring the total volume of oxygen gas that could be produced by the reaction. The ideal gas law gave us the moles of oxygen, which we plugged into the reaction 2 H 2 O 2 (l) 2 H 2 O (l) + O 2 (g) and found the molarity of hydrogen peroxide to be 0.08M. Our experimental value, 0.088M, differed by 9.1%. The experiment relied on certain variables, such as pressure, temperature and concentration, being constant to assist in our calculations. We didn’t achieve constant temperature in several parts and had trouble equalizing the syringe to maintain constant pressure. The majority of the error in our calculations can be accounted for by these factors. Our methods improved and got more accurate as the lab progressed....
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This note was uploaded on 04/08/2008 for the course CHEM Chem 1A taught by Professor Van koppen during the Winter '08 term at UCSB.
- Winter '08
- Van Koppen