Given the following system at equilibrium N2O3(g) NO(g) + NO2(g) ∆H = + 40.5 kJ/mole at 45°C Explain how this system will adjust to the following stresses: addition of 75 moles N2O3(g) halving the volume of the reaction vessel adding 25 atm Argon gas at constant volume decreasing the temperature to 0°C removing NO2 (g) via adsorption onto CaO
Given the following system at equilibrium N2O3(g) NO(g) + NO2(g) ∆H = + 40.5 kJ/mole at 45°C Explain how this system will adjust to the following stresses: addition of 75 moles N2O3(g) halving the volume of the reaction vessel adding 25 atm Argon gas at constant volume decreasing the temperature to 0°C removing NO2 (g) via adsorption onto CaO
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 28PS: Kp for the following reaction is 0.16 at 25 C: 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for...
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Question
- Given the following system at equilibrium
N2O3(g) NO(g) + NO2(g) ∆H = + 40.5 kJ/mole at 45°C Explain how this system will adjust to the following stresses:
- addition of 75 moles N2O3(g)
- halving the volume of the reaction vessel
- adding 25 atm Argon gas at constant volume
- decreasing the temperature to 0°C
- removing NO2 (g) via adsorption onto CaO
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