How The Rate Law And Rate Of Reaction Average Time When Iodine To Disappear

The following observations were observed doing the experiment. The first three mixtures’ reaction average time (for iodine to disappear in the mixture) was similar. Mixture number four reaction average time for iodine to disappear was at least double the first three reaction time, since the amount of iodine was double in this mixture. The reaction rate for mixture number four should also be greater than the reaction rates for the first three mixtures since the average time was larger than the first three mixtures [2]. This chart shows the first, second, and the average time for the mixture’s reaction rates concluded from this experiment. The purpose of this experiment is to determine the rate law and rate constant for the reaction between acetone,
iodine, and hydrochloric acid [1]. The rate law for this experiment was k[acetone][H+] and the average rate constant determined was 3.2 x 10 -5 M-1 s-1. The actual rate law for this experiment is k[acetone][H+]. With this conclusion, the rate law determined for this experiment was the same as the actual rate law.