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Chapter 14 Review

Chapter 14 Review. Determine an average rate and compare relative rates for the reaction: A 2  2 A. What is the average rate of disappearance for t=0min to t=3min? What is the average rate of appearance for the product A from t=3min to t=6min?. Chapter 14 Review.

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Chapter 14 Review

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  1. Chapter 14 Review • Determine an average rate and compare relative rates for the reaction: A2  2 A • What is the average rate of disappearance for t=0min to t=3min? • What is the average rate of appearance for the product A from t=3min to t=6min?

  2. Chapter 14 Review • Given the following set of experiments, determine the Rate Law and value of the rate constant, k.

  3. Chapter 14 Review • Use both the first and second order integrated rate equations. • Ex) The decomposition of ethyl chloride is first order with a rate 2.6 E-3/s. If an initial concentration of 0.0500M decomposes for 5.5 minutes, then how much ethyl chloride remains?

  4. Chapter 14 Review • Given concentration versus time data, determine whether the reaction is first or second order.

  5. Chapter 14 Review • Use the Arrhenius Equation. • Ex) The Activation Energy for a reaction is 55kJ/mol. The rate constant at 298K is found to be 0.25/s. What is the rate constant at 348K?

  6. Chapter 14 Review • Given a mechanism, determine the overall reaction, the rate law, and identify catalysts and reaction intermediates. • Step 1: NO2Cl  NO2 + Cl (slow) • Step 2: NO2Cl + Cl  NO2 + Cl2 (fast)

  7. Chapter 15 Review • Write a K expression for a reaction. • 2 NO(g) + Br2(g)  2 NOBr(g) • Evaluate a K if given equilibrium concentrations. • Ex) At equilibrium, [NO] = 0.050M, [Br2] = 0.075M, and [NOBr] = 0.022M.

  8. Chapter 15 Review • Relate Kc to Kp given one or the other. • For the reaction below, Kc is 1.1 x 10-2 at 300C. What is the value of Kp? • CO(g) + 2H2(g) CH3OH(g)

  9. Chapter 15 Review • Use stoichiometry to find K. • A 1.50L vessel was filled with 0.150 moles of CO and 0.300 moles of H2 and allowed to achieve equilibrium at 500K. At equilibrium, the vessel is found to contain 0.120 moles of CO. What is the equilibrium constant, Kc? • CO(g) + 2H2(g) CH3OH(g)

  10. Chapter 15 Review • Determine an equilibrium concentration from initial amounts. • For the following reaction at 475K, the value of the equilibrium constant is 62. If 0.040 moles of H2 and 0.020 moles of Br2 are added to a 2.0L vessel, then what is the equilibrium concentration of HBr? • H2(g) + Br2(g) 2 HBr(g)

  11. Chapter 15 Review • Calculate a reaction quotient, Q, and determine the direction of movement. • Q > K; reaction shifts to left • Q < K; reaction shifts to right • Q = K; reaction at equilibrium

  12. Chapter 15 Review • Know the effect of LeChatelier’s Principle on a reaction. • N2O4(g) 2 NO2(g) • What happens if: • More NO2(g) is added? • Some N2O4(g) is removed? • The pressure is increased? • If the temperature increase, more NO2(g) is produced. Is the reaction endo- or exothermic?

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