2) Consider the oxidation reaction 1 NO(g) + O₂(g) = NO₂(g) (a) Calculate A,Gº for the oxidation of 1 mole of NO(g) at 25.00 °C and 1.00 bar. (b) Calculate the equilibrium constant K(T) in the conditions of part (a). (c) Estimate the value of the equilibrium constant at T = 40.00 °C and 1.00 bar. (d) State any assumptions that you make. Substance AH(kJ mol−¹)| AƒGº(kJ mol-¹) NO₂(g) NO(g) H₂O(g) H₂O(liq) O₂(g) 33.18 90.25 -241.82 -285.83 0.0 51.47 86.55 -228.57 -237.13 0.0

2) Consider the oxidation reaction 1 NO(g) + O₂(g) = NO₂(g) (a) Calculate A,Gº for the oxidation of 1 mole of NO(g) at 25.00 °C and 1.00 bar. (b) Calculate the equilibrium constant K(T) in the conditions of part (a). (c) Estimate the value of the equilibrium constant at T = 40.00 °C and 1.00 bar. (d) State any assumptions that you make. Substance AH(kJ mol−¹)| AƒGº(kJ mol-¹) NO₂(g) NO(g) H₂O(g) H₂O(liq) O₂(g) 33.18 90.25 -241.82 -285.83 0.0 51.47 86.55 -228.57 -237.13 0.0

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 15P

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