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Unit 7: Kinetics

Unit 7: Kinetics. Microscale Kinetics Collision Theory Day 6. Unit 7: Kinetics. Graphical Determination Review. If given time and reactant conc. data, make 3 graphs …. [R] vs time. ln [R] vs time. 1/[R] vs time. Unit 7: Kinetics. The Microscopic Side of Reaction Rate.

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Unit 7: Kinetics

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  1. Unit 7: Kinetics Microscale Kinetics Collision Theory Day 6

  2. Unit 7: Kinetics Graphical Determination Review If given time and reactant conc. data, make 3 graphs … [R] vs time ln[R] vs time 1/[R] vs time

  3. Unit 7: Kinetics The Microscopic Side of Reaction Rate What is happening on the atomic scale that gives us the different reaction rates we can observe in the real world? NO(g) + O3(g)  NO2 + O2 Rate = k [NO] [O3] What is happening as these gases react?

  4. Unit 7: Kinetics Collision Theory of Reaction Rates 1. The reacting molecules must collide with one another 2. The reacting molecules must collide with sufficient energy to initiate the process of breaking and forming bonds 3. The molecules must collide in an orientation that can lead to the proper rearrangement of products How does this explain the effect of reactant concentration on reaction rate? How does this explain the effect of temperature on rxn rate?

  5. Unit 7: Kinetics 2. The reacting molecules must collide with sufficient energy to initiate the process of breaking and forming bonds

  6. Unit 7: Kinetics 2. The reacting molecules must collide with sufficient energy to initiate the process of breaking and forming bonds Activation Energy, Ea The energy required by reactants in order to initiate the reaction. If the activation energy low… If the activation energy high… Molecular Energy Distribution

  7. Unit 7: Kinetics Activation Energy, Ea Activation energies are frequently represented by energy diagrams or reaction coordinate diagrams Catalysts Catalysts speed up reaction rates by lowering activation energies!!!

  8. Unit 7: Kinetics

  9. Unit 7: Kinetics The Arrhenius Equation Reaction rates depend on the energy and frequency of collisions. Lets summarize that with an equation! Sample problem 1: Plug and chug … don’t waste my time.

  10. Unit 7: Kinetics The Arrhenius Equation Reaction rates depend on the energy and frequency of collisions. Lets summarize that with an equation! Sample problem 1: Plug and chug … don’t waste my time. Sample problem 2: Determining Ea from k at 2 different T’s

  11. Unit 7: Kinetics Sample Problem 2 Use values of k determined at two different temperatures to calculate the value of Ea for the decomposition of HI 2HI  H2 + I2 k1=2.15x10-8 L/(mol s) at 650 K k2=2.39x10-7 L/(mol s) at 700 K

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