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4. free energy

4. free energy. Figure 17.10: Arguably, the most important graph in chemistry. G rxn °. G rxn. G mix °. Use the table below to answer the following questions. 1. Calculate G rxn ° at 298 K for the reaction H 2 (g)+1/2O 2 (g)H 2 O(g) using G f ° values.

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4. free energy

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  1. 4. free energy Chapter 17 Notes

  2. Figure 17.10: Arguably, the most important graph in chemistry. Chapter 17 Notes

  3. Grxn° Grxn Gmix° Chapter 17 Notes

  4. Use the table below to answer the following questions. 1. Calculate Grxn° at 298 K for the reaction H2(g)+1/2O2(g)H2O(g) using Gf° values. 2. Calculate Grxn° at 298 K for the reaction H2(g)+1/2O2(g)H2O(g) using Hf° and S° values. 3. Calculate the equilibrium constant for this reaction at 298K. 4. Calculate the equilibrium constant for this reaction at 1500K. Chapter 17 Notes

  5. 5. Calculate G at 298 K and 1500 K for this reaction when the partial pressure of H2O is 10.0 atm and the partial pressures of H2 and O2 are 0.001 atm. Now interpret your answers by considering the following: 6. What does it mean when Grxn° is negative? positive? 7. Explain how the sign of Grxn° , the size of K, and the extent of reaction at equilibrium are related. 8. Under what conditions, if any, is this reaction spontaneous? nonspontaneous? Explain why for each case by discussing the system and the surroundings. Chapter 17 Notes

  6. Calculate the standard enthalpy, entropy, and free energy change for the Ba(OH)2•8H2O + NH4Cl reaction at 298 K. Go on to calculate the equilibrium constant K for the reaction. Is this reaction spontaneous? Why? Chapter 17 Notes

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