We can use Hess's Law (and some creativity!) to learn about the energetics of reactions that occur in remote environments. Consider the atmospheric reaction, NO + O → NO₂ (a) Use the dissociation energy of O2, 498.34 kJ/mol, and the standard heats of formation for NO (+90.25 kJ/mol) and NO₂ (+33.18 kJ/mol) to derive the enthalpy change for this reaction. QUESTION 14 (b) The two bonds in NO2 are equivalent, and we can use the bond strength of N₂, 945 kJ/mol, and the information given in part (a) to determine ArxnH for N+O+O→ NO₂ From this ArxnH, estimate the bond strength of each of the resulting N-O bonds in kJ/mol. (Note: Your answer for this part does not necessarily depend on your answer to part a).

We can use Hess's Law (and some creativity!) to learn about the energetics of reactions that occur in remote environments. Consider the atmospheric reaction, NO + O → NO₂ (a) Use the dissociation energy of O2, 498.34 kJ/mol, and the standard heats of formation for NO (+90.25 kJ/mol) and NO₂ (+33.18 kJ/mol) to derive the enthalpy change for this reaction. QUESTION 14 (b) The two bonds in NO2 are equivalent, and we can use the bond strength of N₂, 945 kJ/mol, and the information given in part (a) to determine ArxnH for N+O+O→ NO₂ From this ArxnH, estimate the bond strength of each of the resulting N-O bonds in kJ/mol. (Note: Your answer for this part does not necessarily depend on your answer to part a).

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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We can use Hess's Law (and some creativity!) to learn about the energetics of reactions that occur in remote environments. Consider the atmospheric reaction, NO + O → NO2 (a) Use the dissociation energy of O2, 498.34 kJ/mol, and the standard heats of formation for NO (+90.25 kJ/mol) and NO2 (+33.18 kJ/mol) to derive the enthalpy change for this reaction.
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[2] When 1.045 g of CaO is added to 50.0 ml of water at 22.0 °C in a coffee-cup calorimeter, the temperature of the water increases to 29.3 °C. Assume that the specific heat and density of the solution is 4.184 J/g-°C and 1.00g/ml, respectively. The heat capacity of the calorimeter is 18.0 J/°C. Calculate AH for the reaction. CaO(s) + H2O(1) –→ Ca(OH)2(aq); AH =