Understanding The Concept Of Chemical Kinetics Essay
Experiment 10 – Kinetics
TA: Jamie Trindell
April 25, 2016
INTRODUCTION This experiment focused on the concept of chemical kinetics, which describes the speed at which a chemical reaction occurs and the amount of reactant or product remaining after a specific period of time. Kinetics is important in analyzing the rates of certain species and reactions, and is a crucial technique to predict different reactions. Kinetics is a very broad topic, thus the experiment focused only on the derivation of empirical rate laws and their corresponding rate constants. The rate of a specific reaction can be expressed with an experimentally-determined, or empirical, rate law in the form of rate = k[A]x[B]y[C]z. The exponents x, y, and z depend on the term order of each reactant, and the overall order of a reaction. This equation can be derived in different ways, one of which is shown as (rate 1)/(rate 2)= (k[〖KI〗_1 ]^x [〖FeCl3〗_1 ]^y)/(k[〖KI〗_2 ]^x [〖FeCl3〗_2 ]^y ). Also in order to determine the initial concentration of species, the equation m1c1 = m2c2 can be utilized. In this specific experiment, five trials with different concentrations of the two species, KI and FeCl3, are performed.
EXPERIMENTAL To start the experiment, the total amount of the three solutions used in this experiment, KI, FeCl3, and H2O, were gathered. To do this a 3 mL pipette was used to add 9 mL of 0.02 M KI from the stock solution…