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Decomposition of Hydrogen Peroxide Lab

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Purpose To find the activation energy of the following reaction: Data Collection Part 1 Element Molarity 0.88 M (3%) 0.5M Volume Temperature Table 1-Increase in Pressure over Time as 0.88M and 0.5M react at 21.5 Time (s) Pressure (kPa)�0.2% 10 103.6 20 104.0 30 104.0 40 104.0 50 104.5 60 105.4 70 105.9 80 107.0 90 108.6 100 109.7 110 111.1 120 113.4 130 115.4 140 117.2 150 119.3 160 121.8 170 124.0 180 125.9 * Uncertainty of pressure based on instrument stated uncertainty. Sample Calculation Converting Concentration of into Molarity Part 2 Element Molarity 0.88 M (3%) 0.25M Volume Temperature Table 2-Increase in Pressure over Time as 0.88M and 0.25M react at 21.5 Time (s) Pressure (kPa)�0.2% 30 102.0 40 102.2 50 102.7 60 102.9 70 104.5 80 104.5 90 104.7 100 105.6 110 106.3 120 106.5 130 107.0 140 108.1 150 108.8 160 110.0 170 110.6 180 111.3 Qualitative Observations In general for the 4 trials, the following observations were made: * Liquid turned a dark shade of yellow once the reactants were mixed * Once the reactants were mixed, there was a steady increase in bubbling Part 3 Element Molarity 0.44 M (1.5%) ...read more.


Conclusion In conclusion it was found that the activation energy of the decomposition of hydrogen peroxide with the help of the catalyst KI is . When compared to an actual value there was a percent difference of 43%. In fact the actual value that was used is the activation energy of hydrogen peroxide in the absence of a catalyst. So in reality it is likely that a catalyst would cause the activation energy to be even smaller, and the percent difference would be even greater. The only reasonable explanation as to why the calculated activation energy is so much greater is that somewhere during the experiment a random error occurred but since only two trials were done, it is impossible to pinpoint where it exactly occurred. When looking at graphs 1-4 it can be seen that as time went on the pressure increased exponentially. This makes sense because over time the amount of gas increased, and so the pressure would increase too. In addition in graphs 1-4, if a curved line of best fit were to be plotted, than the y-intercept would show the pressure of the room at the moment the experiment was conducted. ...read more.


Lastly, when the test tube was put in the water bath, the temperature of the water bath was constantly changing because the temperature of the water was relatively lower than the room temperature. This in turn is what caused fluctuation in the temperature readings. This in turn could have also caused the initial rate to vary because as discussed earlier, even the slightest change in temperature causes the initial rate to change. This experiment can be improved in many ways. One of the main things that can be done is that the experiment should be conducted at different temperatures so that at least a minimum of 5 k values against 1/T can be plotted on graph 5. In addition, the temperature increments should have a relatively broad range, which in turn will make the data and the trends clearer. In addition, the experiment should be conducted on the same day so as the temperature can be kept constant for certain k values. In order to keep the temperature of the water bath constant, the experiment should be conducted in a closed environment so that less energy is lost to the environment. ...read more.

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