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Conclusion:
The graphs and data in the table shows that there is a pattern between increasing the temperature and increasing rate of reaction (decrease in time taken for reaction) between sodium thiosulfate and hydrochloric acid molecules. Therefore increasing temperature results in more molecules having greater kinetic energy and thus more collisions per unit time. In addition, increasing temperature results in more molecules having energy greater than that of the activation energy, thus resulting in more successful collisions. Hence my hypothesis has been proved correct, “Increasing the temperature (oC) will lead to a decrease in the time taken (seconds) for reaction between sodium thiosulfate and hydrochloric acid molecules to occur.”

Discussion:
Scatter and Precision:
From the graphs it is plain that there is a scatter of results both above and below the curve (line of best fit). This scatter of results is mainly due to the degree of random error that could have occurred during the practical. These random errors could have caused the experiments final results to be less precise and therefore the results are slightly scattered, but a clear residual pattern still exists on the graphs.

Random and Systematic Errors:
During this experiment there was some degree of error present which contributed to fluctuations of the final results. The types of errors that could have occurred are either random errors (experimenters fault – “incorrect judgments made by the experimenter”) or systematic errors (faults in equipment used). Random errors contribute to making results less precise, while systematic errors contribute towards the final results to be less accurate.
The possible random errors that could have occurred in this practical are incorrect judgement of temperature on the thermometer, incorrect timing of the formation of the precipitate, incorrect judgement of the disappearance of the cross due to...