Hydrogen Peroxide Decomposition Lab Report

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The purpose of this experiment was to analyze the rate of the catalyzed decomposition of hydrogen peroxide in regard to the effects of concentration and temperature.
2H2O2 (l) —I-—> 2H2O (l) + O2 (g) In part one of the experiment, catalyst KI was added to varying solutions of 3% hydrogen peroxide and DI water and the composition of hydrogen peroxide was observed. This was observed by collection the volume of oxygen gas produced during the decomposition, and measuring its volume. From that, volume of oxygen gas produced was plotted against time and a linear least square fit line was generate. From the line equation, rate was derived, rate is equal to the slope of the line. This procedure was repeated for two other solutions, generating three sets of results and three separate rates. The order of the each reactant, hydrogen peroxide and KI, was determined by creating a table that contained the volume of each reactant in each solution and the rate from the line equation. From this the
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The reaction was allowed to continue for twenty minutes and the volume of oxygen gas produced was measured. The decomposition of hydrogen peroxide is a very slow process; however, with the addition of the catalyst, KI, the reaction rate is increased and the decomposition occurs much quicker. The partial pressure of oxygen gas was calculated using the barometric pressure and the vapor pressure of water. From this the moles of I- were calculated and found to be 0.005 moles I-. The solution was then titrated with AgNO3 and volume used to generate the colour change was recorded. From the volume of AgNO3 used for the titration, the moles of Ag+ were calculated and found to be 0.005 moles of Ag+. Silver ions and iodine ions react in mole ratio of 1:1 to form the precipitate AgI (s). From the mole ratio it was calculated that 0.005 moles of I- reacted and thus 100% of I- was

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