Investigating The Relationship Between Temperature And The Rate Of Reaction Of Iron

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Discussion This experiment investigated the relationship between temperature and the rate of reaction of iron (III) nitrate reacting with sodium thiosulfate. The results show the rate of iron (III) forming iron (II) increases as the temperature of the solutions increase. When the temperature of the reactants is 4℃, it takes 54.173 seconds for the reaction to occur until the cross appears (Table 1). The time taken to reach the same transparency reduces to 16.37 seconds at 25℃ and to 2.09 seconds at 65℃. The line of best fit in Graph 1 suggests an inverse relationship between temperature and reaction time. The results for the rate of reaction, seen in Table 2, suggest that as the temperature increases, the rate of reaction increases at a…show more content…
This increased as the temperature was changed, with the percentage range rising from 8.77% to 10.2% as it cooled, and from 24% and 42% when the solutions were heated. This suggests that there was random error produced from the cooling process, and more significantly in the heating process. A source of error in the heating and cooling process was the uneven distribution of heat in the hot water bath. The solution was said to be at the desired temperature when the sodium thiosulfate was measured to be at that temperature. The temperature of iron nitrate was not measured, but assumed to be equal to that of the sodium thiosulfate, even though the sodium thiosulfate, at one point, was observed to have a greater temperature than the water bath, implying uneven heating. This was a procedural error as the uneven heating may have led to different temperatures of iron nitrate, producing random error as different temperatures of the iron nitrate would lead to different rates of reactions. Moreover, the temperature of the solutions that were cooled in test tubes were not measured, as this would delay the procedure and introduce more random error. The high surface area of the test tubes allowed faster cooling of the liquid to the temperature of the water bath, so were assumed to be at the same temperature as the water bath. This assumption, if incorrect, would have led to systematic error where the temperatures were consistently higher than the actual temperature of the solution,

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