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For the reaction 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂(g) AH = -81.1 kJ and AS = -1.20 J/K The equilibrium constant for this reaction at 308.0 K is Assume that ΔΗ° and AS are independent of temperature.

For the reaction 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂(g) AH = -81.1 kJ and AS = -1.20 J/K The equilibrium constant for this reaction at 308.0 K is Assume that ΔΗ° and AS are independent of temperature.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.79QP: Use thermochemical data (Appendix C) to decide whether the equilibrium constant for the following...
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For the reaction 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂ (g) AH° -81.1 kJ and AS⁰ = - - 1.20 J/K The equilibrium constant for this reaction at 308.0 K is Assume that ΔΗ° and AS are independent of temperature.
Transcribed Image Text:For the reaction 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂ (g) AH° -81.1 kJ and AS⁰ = - - 1.20 J/K The equilibrium constant for this reaction at 308.0 K is Assume that ΔΗ° and AS are independent of temperature.
For the reaction N₂ (g) + O₂(g) → 2NO(g) 181 kJ and AS⁰ = 24.9 J/K The equilibrium constant for this reaction at 327.0 K is ΔΗ° = Assume that ΔΗ° and AS are independent of temperature.
Transcribed Image Text:For the reaction N₂ (g) + O₂(g) → 2NO(g) 181 kJ and AS⁰ = 24.9 J/K The equilibrium constant for this reaction at 327.0 K is ΔΗ° = Assume that ΔΗ° and AS are independent of temperature.
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