Rate Law for the Crystal Violet Reaction
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The aim of this experiment was to basically demonstrate how a common integer rate can be established irrespective of the condition of the reactants. The rate law reaction as expressed in the equation shows the point of convergence between the stoichiometric coefficients and the reaction orders. It is important to remember that the general rate law of the reaction may be used to calculate the constants for any 2 adjacent data points.
Looking at the results, it is evident that there was enough time for carrying out the experiment more than once. The relevance and validity of the calculated values of k and OH between the two experiments confirms the fact that the method used in the trial was valid. However, one must keep in mind that experiments of this nature are prone to errors. Crystal violet has attendance of degrading with time. It is difficult to ascertain the freshness of the crystal violet in experiments of this nature. However, based on the trial results that involved 0.2M NaOH, it can be concluded that the state of the crystal violet was fresh. Another probable source of error is the procedure in which the reagents and mixtures were prepared. The experiment used limited doses of the reaction mixtures. This is only possible if used in small containers, such as test tubes. Test tubes cannot provide the volume required to stir the reagents properly.
Finally, closer attention must be paid to the calorimeter. In the preparation of equipments, the calorimeter was calibrated before it was used. This poses the danger of minor software flaws and undetected smears that have a bearing to the eventual outcome of the experiment. Experiments of this nature are extremely sensitive to errors that cannot be seen with a naked eye. Therefore, one must be extremely cautious during experiment time.