Consider the system of a gaseous mixture of N2, O2, NO, and NO a) [3 pts]...

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Consider the system of a gaseous mixture of N2, O2, NO, and NO₂ a) [3 pts] How many degrees of freedom does this system have? b) [1 pts] Are the following two reactions reasonable? (1) N2(g) + O2(g) → NO(g) (2) N2(g) + O2(g) → NO2(g) c) [3 pts] Assuming the reactions are reasonable for the system, express the equilibrium mole fractions in terms of the reaction coordinates. d) [3 pts] At equilibrium, given the following information of the system, compute the mole fractions of NO and NO₂ T = 2000 K P = 200 bar K₁ = 2.004 x 10-² YN₂ = 0.70 Yo₂ = 0.05 K₂ = 6.9373 x 10-5 e) [Bonus 1 pt] What is the link with the presentation of Aera on June 2? Why is this reaction equilibrium important? Consider the system of a gaseous mixture of N2, O2, NO, and NO₂ a) [3 pts] How many degrees of freedom does this system have? b) [1 pts] Are the following two reactions reasonable? (1) N2(g) + O2(g) → NO(g) (2) N2(g) + O2(g) → NO2(g) c) [3 pts] Assuming the reactions are reasonable for the system, express the equilibrium mole fractions in terms of the reaction coordinates. d) [3 pts] At equilibrium, given the following information of the system, compute the mole fractions of NO and NO₂ T = 2000 K P = 200 bar K₁ = 2.004 x 10-² YN₂ = 0.70 Yo₂ = 0.05 K₂ = 6.9373 x 10-5 e) [Bonus 1 pt] What is the link with the presentation of Aera on June 2? Why is this reaction equilibrium important?