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General Chemistry II Workshop 13: Kinetics part 2 (A graphical analysis) By now you know that thermodynamics helps us to predict whether or not a process will be spontaneous at given conditions and kinetics tells us whether or not a thermodynamically allowed process will actually proceed at a measurable rate under these conditions. The rate at which a reaction will proceed is determined by its activation energy, Ea. Activation energy can be defined as the energy necessary to initiate an otherwise spontaneous chemical reaction so that it will continue to react without the need for additional energy. (For example burning paper -- the reaction of cellulose and oxygen is spontaneous, but you need to initiate the combustion by adding activation energy from a lit match). You can use graphical analysis methods to determine the activation energy of a chemical reaction. In this workshop we will use experimental results in form of graphs to obtain information about kinetics of two chemical processes. Part 1: Integrated rate laws Read the graph below and without doing any calculation answer the following questions. Before you write down your answers make sure that everyone in your group agrees with them. 2 HI(g) → H₂(g) + I2(g) P is a partial pressure of HI(g) in atm 6.20 6.00 In P vs. time 5.80 5.60 5.40 5.20 y = -1.19E-04x + 5.99E+00 5.00 4.80 8000 10000 드 0 2000 4000 6000 time (s) 12000
General Chemistry II Part 2: Concentration V time plot 1. Consider the 1st order decomposition of hydrogen iodide and using the graph below answer the questions that follow. The data in the graph was collected at 298K. 2 HI(g) → H₂(g) + I2(g) 0.06 0.05 0.04 0.03 0.02 0.01 0 0 50 100 150 200 250 300 350 400 450 500 Time (s) a) What is the numerical value of the rate constant for this 1st order reaction? b) What would the rate be if the concentration of HI was 1.80 M? c) Calculate how much time it takes for the concentration of hydrogen iodide to decrease from 0.050M to 0.00150M at 298K.
General Chemistry II d) If you raise the temperature to 318 K, you find the rate of the reaction has increased by a factor of 4.4. What is the activation energy for this reaction? e) You conduct another experiment at 298K in which you use a catalyst to speed up the reaction. If the rate of the reaction goes up by a factor of 20 what is the change in activation energy for this experiment? 5