Chapter 14- Arrhenius Equation Supplemental Instruction Iowa State University Leader: Seth Course: Chem 178 Instructor: Dr. Kingston Date: Wednesday, 2/3/10 Announcements 1. Go around question- Bouncy ball or slinky? 2. Exam I Review Monday, 2/8/10- 5:10 to 7:00 pm in 1213 Hoover Agenda: Go over Exam 1 from Spring 2008 and answer questions Warmup- Working with exponential functions For the Arrhenius equation below, identify the variables and units Take the natural logarithm of both sides of the Arrhenius equation. (If you plot ln k vs. 1/T the slope of your line should be –Ea/R.) Problems 1. Calculate the fraction of atoms in a sample of argon gas at 400K that have an energy of 10.0 kJ/mol or greater. 2. The decomposition of NO to N2 and O2 is second order with a rate constant of 0.796 M-1s-1 at 737oC and 0.0815 M-1s-1 at 947oC. Calculate the activation energy for the reaction.3. The activation energy of a certain reaction is 65.7 kJ/mol. How many times faster will the reaction occur at 50oC than at 0oC? 4. The decomposition of HI has rate constants k = 0.079 M-1s-1 at 508°C and k = 0.24 M-1s-1 at 540°C. What is the activation energy of this reaction in kJ/mol? At home: The reaction 2NO2 → 2NO + O2 has an activation energy of 111 kJ/mol. At 400°C, k = 7.8 M-1s-1. What is the value of k at 430°C? Wrap up- round robin Write down what you learned
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