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3. What is the equilibrium constant for the decomposition of Nitric Oxide at 25 °C, given that AG of NO= -867 kJ/mol.? 2NO(g) = N₂(g) + O₂(g)

3. What is the equilibrium constant for the decomposition of Nitric Oxide at 25 °C, given that AG of NO= -867 kJ/mol.? 2NO(g) = N₂(g) + O₂(g)

Chemistry
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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Module 13 Homework 1. For the following reaction calculate AS°, AH, and AG at 25 °C. MgCO3(s) MgO(s) + CO₂(s) Compound MgCO3 (s) MgO (s) CO₂ (g) AH,° -1112.9 kJ/mol -601.8 kJ/mol -393.51 kJ/mol b. Endothermic Reaction 2. What must the sign of the change in enthalpy be for each scenario? Which is most likely to be more thermodynamically stable for each scenario: products or reactants and why? a. Exothermic Reaction SP 65.69 J/mol K 26.78 J/mol*K 213.8 J/mol K 3. What is the equilibrium constant for the decomposition of Nitric Oxide at 25 °C, given that AG of NO= -867 kJ/mol.? 2NO(g) = N₂(g) + O₂(g) 311
Transcribed Image Text:Module 13 Homework 1. For the following reaction calculate AS°, AH, and AG at 25 °C. MgCO3(s) MgO(s) + CO₂(s) Compound MgCO3 (s) MgO (s) CO₂ (g) AH,° -1112.9 kJ/mol -601.8 kJ/mol -393.51 kJ/mol b. Endothermic Reaction 2. What must the sign of the change in enthalpy be for each scenario? Which is most likely to be more thermodynamically stable for each scenario: products or reactants and why? a. Exothermic Reaction SP 65.69 J/mol K 26.78 J/mol*K 213.8 J/mol K 3. What is the equilibrium constant for the decomposition of Nitric Oxide at 25 °C, given that AG of NO= -867 kJ/mol.? 2NO(g) = N₂(g) + O₂(g) 311
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