4. Use tabulated bond energies to estimate the enthalpy of reaction for each of the following gas phase reactions. a. N₂ + 3H₂ → 2NH3 b. CO + H2O > CO2 + H2 5. Assuming that the gases are ideal, calculate the amount of work done (in joules) in the following reaction. Is the work done on or by the system? Consider the oxidation of one mole of HCl(g) at 200°C. 4HCl(g) + O₂(g) 2Cl₂(g) + 2H₂O(g) 6. Use data in Appendix K to find the enthalpy (AHº), entropy (AS°), and AG° of reaction for the following. Indicate whether the reaction is spontaneous or non-spontaneous. a. NH4NO3(s) → N₂O(g) + 2H₂O(1)

4. Use tabulated bond energies to estimate the enthalpy of reaction for each of the following gas phase reactions. a. N₂ + 3H₂ → 2NH3 b. CO + H2O > CO2 + H2 5. Assuming that the gases are ideal, calculate the amount of work done (in joules) in the following reaction. Is the work done on or by the system? Consider the oxidation of one mole of HCl(g) at 200°C. 4HCl(g) + O₂(g) 2Cl₂(g) + 2H₂O(g) 6. Use data in Appendix K to find the enthalpy (AHº), entropy (AS°), and AG° of reaction for the following. Indicate whether the reaction is spontaneous or non-spontaneous. a. NH4NO3(s) → N₂O(g) + 2H₂O(1)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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