CHM480 Chapter Notes - Chapter 1-10: Iodine Test, Reaction Rate, Filter Paper
Document Summary
Experiment 1 - activation energy for the acid-catalysed hydrolysis of ethyl- acetate/methyl acetate. Hcl (0. 5n), ethyl acetate/methyl acetate, (0. 2n) naoh, phenolphthalein indicator, (0. 2n) oxalic acid, distilled water. Theory: the overall reaction is represented as, it is a pseudo first order reaction and follows the rate law, rate=k [ester], where k=k" [h2o] [h+], k and k" being the true and apparent rate constants respectively. Here, k"= (2. 303/t) log [a/(a-x)] where a and (a-x) are the concentrations of the ester at zero and at a given time t" from the start of the reaction. The activation energy is the energy required to form the activated complex from the reactants. Ea is related to rate constant by arrhenius equation as, log k=log a- ea/(2. 303rt) Therefore, from the slope of the straight line generated by plotting the log k values against 1/t, the value of ea can be obtained.
