9. Analyze the data and retrieves the initial rate(slope) from the linear regression. Data: Fig.1. Shows the pressure and temperature recorded before mixing. Fig. 2. Shows the temperature and pressure after mixing Part Reactants Temperatur e (ᵒC) Initial rate (kPa/s) I 4 mL 3.0% H 2 O 2 + 1 mL 0.5 M KI 18.1 ᵒC 116.14 kPa Part Volume H 2 O 2 ( mL) (H 2 O 2 ) before mixing Volume KI (mL) (KI) before mixing
I 4 0.882 M 10.50 M 0.50 M Fig. 3. Fig. 4 Fig. 5.
Discussion: My data was good because, during the Part I of a four-part lab experiment where we were instructed to carry out the decomposition of hydrogen peroxide using a catalyst 0.5 M of KI solution at 20 C. We first measured the temperature of the water bath which recorded to be at ᵒ 18.1 C. I predicted the water temperature to remain constant throughout the entire experiment, ᵒ but in this instance, it was perfect to carry out the decomposition process. We then added 4 mL of H 2 O 2 into the test tube which was then submerged into the water bath. A 2 mL of 0.5 M KI solution was measured out, where 1 mL of the KI solution was added to the hydrogen peroxide H 2 O 2 solution 0.5 M of the catalyst potassium iodide solution was used because the lower the concentration it produces a reaction which lasts a few minutes exactly what was needed. If a reaction is less than a few minutes, it becomes hard to see how it progresses over a certain time-span and if a reaction is more than few minutes it is time wasting. Once both solutions were combined, the temperature was still stabilized, and a pressure of 116.14 kPa was recorded. Hydrogen peroxide decomposition at a slower rate on its own, but with the presence
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- Fall '19