The results of the lab show the decomposition rate of H2O2 at various amounts of KI, H2O, and H2O2. In addition, the effect of temperature on the rate of the reaction can also be seen in the results.
Figure 1 Figure 2
`Figure 3
Figures 1,2 and 3 represent the results obtained from the keeping the amount of KI constant and varying the amount of H2O2 and water. It can be seen that when H2O2 is doubled (Figure 1 to Figure 2) the rate is also doubled from 0.0368 mL/s to 0.0723 mL/s. When the amount of H2O2 increases by 5 mL (Figure 2 to Figure 3) it again increases about 0.04 mL/s.
Figure 4 Figure 5
Figure 6
Figures 4, 5, and 6 represent the data collected when the amount of H2O2was held constant while the amount of KI and water is …show more content…
The results showed that the highest rate of reaction occurred when there was 10.0 mL of KI and 15.0 mL of H2O2 and no water mixed, this is seen in Figure 2. The lowest rate of reaction occurred, when the least amount of H2O2 was added, this is represented in Figure 1. When it comes to how the temperature affected the rate, the higher temperature of 31.5°C had a greater rate than the temperature that was 5°C less. Based on these observations, we can determine that by increasing the amount of I- increases the rate of the reaction, while increasing the temperature also increases the rate of the reaction. The reason I- increases the rate of the reaction because it is a catalyst and it lowers the activation energy, which allows the reaction to occur faster. This result can be supported by a study that was done on hydrogen peroxide, which determined that H2O2 decomposition increased with temperature and catalyst loading (Shang, Noel, & Hessel, 2017). In addition, using the data collected the order with respect to [H2O2] and with respect to [I-] was determined and found to be first order for each, meaning the overall order of the reaction was second order. Additionally, a solution that is second order means that the rate of reaction is directly proportional to the concentration of the reactant. Furthermore, the molarity of the unknown solution was also able to be determined using the rates found for Run 2 and Run 7 and the rate law that was found for Run
Figure 1 Figure 2
`Figure 3
Figures 1,2 and 3 represent the results obtained from the keeping the amount of KI constant and varying the amount of H2O2 and water. It can be seen that when H2O2 is doubled (Figure 1 to Figure 2) the rate is also doubled from 0.0368 mL/s to 0.0723 mL/s. When the amount of H2O2 increases by 5 mL (Figure 2 to Figure 3) it again increases about 0.04 mL/s.
Figure 4 Figure 5
Figure 6
Figures 4, 5, and 6 represent the data collected when the amount of H2O2was held constant while the amount of KI and water is …show more content…
The results showed that the highest rate of reaction occurred when there was 10.0 mL of KI and 15.0 mL of H2O2 and no water mixed, this is seen in Figure 2. The lowest rate of reaction occurred, when the least amount of H2O2 was added, this is represented in Figure 1. When it comes to how the temperature affected the rate, the higher temperature of 31.5°C had a greater rate than the temperature that was 5°C less. Based on these observations, we can determine that by increasing the amount of I- increases the rate of the reaction, while increasing the temperature also increases the rate of the reaction. The reason I- increases the rate of the reaction because it is a catalyst and it lowers the activation energy, which allows the reaction to occur faster. This result can be supported by a study that was done on hydrogen peroxide, which determined that H2O2 decomposition increased with temperature and catalyst loading (Shang, Noel, & Hessel, 2017). In addition, using the data collected the order with respect to [H2O2] and with respect to [I-] was determined and found to be first order for each, meaning the overall order of the reaction was second order. Additionally, a solution that is second order means that the rate of reaction is directly proportional to the concentration of the reactant. Furthermore, the molarity of the unknown solution was also able to be determined using the rates found for Run 2 and Run 7 and the rate law that was found for Run