Discussion
As a result of the calculations made above, considering the overall; CH3COCH3 (aq) + I2 (aq) + HCl (aq) CH3COCH2I (aq) + HI (aq) the rate law for this reaction is, Rate = k[CH_3 COCH_3 ]^m [I_2 ]^n [HCl]^p. As supported in question 3 part A, the reaction orders m, n and p for acetone, iodine and HCL, respectively were 1, 0, 1. Resulting in an overall reaction order of 2. Manipulations were based on the usage of initial concentrations to calculation the rate constant for the reactions A-D with those values the average rate constant was calculated to be 2.0 x 10-5 M-1s-1. Furthermore, the initial absorbance reading of Crystal Violet in trial 1 and 2 was 1.090 and 1.100, respectively and the reaction order with respect to crystal violet was first order. It was determined to be first order based on the rationale that the correlation coefficient was the closest to 1 in figures 3 and 4. Successively, out of all the three graphs (abs vs. time, ln(abs) vs. time, and …show more content…
As mentioned in part A, the solutions were measured using a graduated cylinder. Due to procedural errors the usage of a graduated cylinder to measure the volume of the liquid reactants had proven to be a source of error. This variability is noticed in table 1; since, at times there is a vast difference in the time it takes the mixture to appear clear for each trial. Although, the procedure mentioned to approximately measure certain amounts of reactant to later solve for initial concentration the graduated cylinder was not the most reliable instrument to measure the volume of liquids accurately. It was also important to note that in a dilution calculation, concentration and volume are inversely proportional to one another. If there’s an increase in volume, then there is a decrease in concentration, vice
As a result of the calculations made above, considering the overall; CH3COCH3 (aq) + I2 (aq) + HCl (aq) CH3COCH2I (aq) + HI (aq) the rate law for this reaction is, Rate = k[CH_3 COCH_3 ]^m [I_2 ]^n [HCl]^p. As supported in question 3 part A, the reaction orders m, n and p for acetone, iodine and HCL, respectively were 1, 0, 1. Resulting in an overall reaction order of 2. Manipulations were based on the usage of initial concentrations to calculation the rate constant for the reactions A-D with those values the average rate constant was calculated to be 2.0 x 10-5 M-1s-1. Furthermore, the initial absorbance reading of Crystal Violet in trial 1 and 2 was 1.090 and 1.100, respectively and the reaction order with respect to crystal violet was first order. It was determined to be first order based on the rationale that the correlation coefficient was the closest to 1 in figures 3 and 4. Successively, out of all the three graphs (abs vs. time, ln(abs) vs. time, and …show more content…
As mentioned in part A, the solutions were measured using a graduated cylinder. Due to procedural errors the usage of a graduated cylinder to measure the volume of the liquid reactants had proven to be a source of error. This variability is noticed in table 1; since, at times there is a vast difference in the time it takes the mixture to appear clear for each trial. Although, the procedure mentioned to approximately measure certain amounts of reactant to later solve for initial concentration the graduated cylinder was not the most reliable instrument to measure the volume of liquids accurately. It was also important to note that in a dilution calculation, concentration and volume are inversely proportional to one another. If there’s an increase in volume, then there is a decrease in concentration, vice