Iodine Clock Reaction Essay
CONCLUSION
The experimentally obtained data collected for the reaction between IO3- and HSO3- at various temperatures is clearly supported by the Arrhenius equation. Referring to Graph 1.7, the line of best fits clearly passes through most of the data points displaying a linear relationship between temperature and the rate of the reaction. The R-squared of the graph which is a statistical measure of how close the data are to the fitted regression line is 0.9818. This number is extremely low which indicates that the data points are very close to the theoretically derived calculations.
Looking at Graph 1.6, it can be said with confidence that the rate of the reaction is directly proportional to the approximate temperature. For e.g. At 15 °C, …show more content…
Due to the lack of literature value for the effects of temperature on the rate of the Iodine Clock Reaction, there was no final percentage error. However, Looking at Graph 1.6, the line of best fits clearly shows the low precision throughout this experiment resulting in an increase of Random error.
This could be due to the many assumptions being made in this experiment. We are assuming that there was no cross contamination between Solution A, B and water. Though it is highly likely that someone used the same pipette or measuring cylinder to measure chemicals as all three solutions were clear and colourless as notes in the overall observations. This could affect the content of each of the beakers as it would change the concentrations and/or volume of the solutions which was to be kept constant (refer to Table 1.1) greatly affecting the data obtained.
It was also assumed that both Sol.A and Sol.B beakers were exactly at the same temperature when the reaction occurred. Even though the temperatures of both beakers were recorded, it was highly likely that the temperature increased or decreased between the time when they were taken out of the water baths and the time they were mixed together. Though this would not be a primary source if error, nonetheless, it can account for a very small part of the experimental
The experimentally obtained data collected for the reaction between IO3- and HSO3- at various temperatures is clearly supported by the Arrhenius equation. Referring to Graph 1.7, the line of best fits clearly passes through most of the data points displaying a linear relationship between temperature and the rate of the reaction. The R-squared of the graph which is a statistical measure of how close the data are to the fitted regression line is 0.9818. This number is extremely low which indicates that the data points are very close to the theoretically derived calculations.
Looking at Graph 1.6, it can be said with confidence that the rate of the reaction is directly proportional to the approximate temperature. For e.g. At 15 °C, …show more content…
Due to the lack of literature value for the effects of temperature on the rate of the Iodine Clock Reaction, there was no final percentage error. However, Looking at Graph 1.6, the line of best fits clearly shows the low precision throughout this experiment resulting in an increase of Random error.
This could be due to the many assumptions being made in this experiment. We are assuming that there was no cross contamination between Solution A, B and water. Though it is highly likely that someone used the same pipette or measuring cylinder to measure chemicals as all three solutions were clear and colourless as notes in the overall observations. This could affect the content of each of the beakers as it would change the concentrations and/or volume of the solutions which was to be kept constant (refer to Table 1.1) greatly affecting the data obtained.
It was also assumed that both Sol.A and Sol.B beakers were exactly at the same temperature when the reaction occurred. Even though the temperatures of both beakers were recorded, it was highly likely that the temperature increased or decreased between the time when they were taken out of the water baths and the time they were mixed together. Though this would not be a primary source if error, nonetheless, it can account for a very small part of the experimental