You are studying the kinetics of the reaction H2(g) 1

Chapter 15, Problem 15.134

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You are studying the kinetics of the reaction H2(g) 1 F2(g) n 2HF(g) and you wish to determine a mechanism for the reaction. You run the reaction twice by keeping one reactant at a much higher pressure than the other reactant (this lower-pressure reactant begins at 1.000 atm). Unfortunately, you neglect to record which reactant was at the higher pressure, and you forget it later. Your data for the first experiment are as follows: Pressure of HF (atm) Time (min) 0 0 0.300 30.0 0.600 65.8 0.900 110.4 1.200 169.1 1.500 255.9 When you run the second experiment (in which the higher-pressure reactant is run at a much higher pressure), you determine the values of the apparent rate constants to be the same. It also turns out that you find data taken from another person in the lab. This individual found that the reaction proceeds 40.0 times faster at 558C than at 358C. You also know, from the energylevel diagram, that there are three steps to the mechanism, and the first step has the highest activation energy. You look up the bond energies of the species involved and they are (in kJ/mol): HOH (432), FOF (154), and HOF (565). a. Sketch an energy-level diagram (qualitative) that is consistent with the one described.