Determining The Mass Percent Of Through The Volumetric Analysis Method
H_2 The purpose of this experiment is to determine the mass % of through the Volumetric Analysis method. To attain this purpose, a decomposition reaction was performed, which can be separated into two steps. First, 2 mL of was reacted with approximately .5 g of KI in an Erlenmeyer flask to form and a hypoiodite species. The second step is the reaction between another molecule of and hypoiodite, which results in reformation of the catalyst, potassium iodide. The catalyst is used to speed up the reaction by decreasing the activation energy. In addition, the catalyst can regenerate itself to be used again till the reaction runs to completion. Overall, the reaction is (l). Oxygen gas will be collected over water through 2 burets. The
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When the potassium iodine was pour into the flask containing , oxygen gas was quickly formed. Since there was a delay in putting the stopper onto the flask in order to have all the potassium iodine pour in, some gas have escaped. This mean the volume of gas would be less, which affected our calculations for mass . Since the catalyst potassium iodine can regenerate itself, it did not matter if all .5 g of catalyst was pour into the flask. Therefore, the data would be more accurate if the stopper would be placed onto the flask immediately after pouring in the catalyst or noticing bubbles generated. The bubbles generated in the flask are oxygen gases. Another system error was not dispensing exactly 2 mL on the third trial. This was important because Since only 1.88 mL of was dispensed, the volume of generated will be less. This also increased the standard deviation in the data. For future trials, the graduated pipet should be used more efficiently and accurately to attain the necessary amount of reactants. Lastly, there was a random error with measuring the temperature of the solution. Throughout the three trials, the temperature was inconsistent. As seen in table 1, the temperature varies from 23.8,22.4, and 22.0. This fluctuation in temperature was not
When the potassium iodine was pour into the flask containing , oxygen gas was quickly formed. Since there was a delay in putting the stopper onto the flask in order to have all the potassium iodine pour in, some gas have escaped. This mean the volume of gas would be less, which affected our calculations for mass . Since the catalyst potassium iodine can regenerate itself, it did not matter if all .5 g of catalyst was pour into the flask. Therefore, the data would be more accurate if the stopper would be placed onto the flask immediately after pouring in the catalyst or noticing bubbles generated. The bubbles generated in the flask are oxygen gases. Another system error was not dispensing exactly 2 mL on the third trial. This was important because Since only 1.88 mL of was dispensed, the volume of generated will be less. This also increased the standard deviation in the data. For future trials, the graduated pipet should be used more efficiently and accurately to attain the necessary amount of reactants. Lastly, there was a random error with measuring the temperature of the solution. Throughout the three trials, the temperature was inconsistent. As seen in table 1, the temperature varies from 23.8,22.4, and 22.0. This fluctuation in temperature was not