Rate Of Reaction Experiment

Rate of Reaction Experiment
Rate of reaction is a term used to measure the time or speed that the reaction occurs in. A rate of reaction can be effected by different factors, such as the concentration, temperature, whether or not a catalyst is involved, the state that the reactants were in at the time of the experiment and the amount of pressure that was involved in the experiment. If the concentration, temperature and the amount of pressure involved were higher than the rate of reaction would be higher. Those factors would affect the speed and the amount the atoms are moving at therefore effecting the amount that the particles collide and hence impacting the rate of reaction.
The two reactants involved in the experiment are Sodium Thiosulfate

The effect of temperatures on rate of reaction

Temperature (degrees Celsius) Room temperature 35 50
Rate of reaction (seconds) 69 56.03 53.63
Table 2: The effect of temperatures when the temperatures were above room temperature. Graph 1: The graph of the results from table 1 Graph 2: The graph of the results from table 2
The results displayed in all the graphs and tables had shown a decrease in time for the rate of reaction, as the temperature increases. The results support the idea that as the temperature of the solution increases, the time, the rate of reaction, decreases.
The results of the experiment had fluctuated based on the temperature of the solution. In reference to Table 1 and Table 2, the results was evident enough to identify the patterns and the trends when it came to using the temperature as an independent variable. The results predicted a trend that the higher the temperature, the higher the rate of reaction is. Whereas, the lower the temperature slowed down the rate of reaction. The trend states that the higher the temperature correlates to a higher rate of

An error that occurred was the concentration of the solvent. Since there were two different dilution of the solution, the amount of water used was different, causing a different concentration and producing a different result. The amount of water used should be measured beforehand to reduce the random error and increase the precision of the results. A systematic error may have been the Bunsen burner being on safety flame instead of a blue flame. The long exposure to the low heat evaporated the water, thus increasing the concentration of Sodium Thiosulfate. The accuracy of the results was changed with the altered concentration. To increase the accuracy of the results, the blue flame should have been used to make the solution reach the temperature needed quicker. This would allow the Sodium Thiosulfate and the Hydrochloric acid to mix in a longer duration of