3. The following question is based on the chemical equilibrium shown below: (13 mins) NO2(g) = N₂O4(g) (UNBALANCED EQUATION). A. Kp for this reaction is 9.3 x 10-7 at 25°C. What is the equilibrium concentration of N₂O4 in a flask that initially contains only 3.00 atm of NO₂? If any assumptions are made for your calculations, please state them and validate their use. B. What is the value of Kc for this reaction at the same temperature? C. What is the effect on Kp if 1.00 atm of neon gas is added to the system a equilibrium? Useful info: Kp = Kc(RT)An R = 0.08206 (L x atm)/ (mol x K)

3. The following question is based on the chemical equilibrium shown below: (13 mins) NO2(g) = N₂O4(g) (UNBALANCED EQUATION). A. Kp for this reaction is 9.3 x 10-7 at 25°C. What is the equilibrium concentration of N₂O4 in a flask that initially contains only 3.00 atm of NO₂? If any assumptions are made for your calculations, please state them and validate their use. B. What is the value of Kc for this reaction at the same temperature? C. What is the effect on Kp if 1.00 atm of neon gas is added to the system a equilibrium? Useful info: Kp = Kc(RT)An R = 0.08206 (L x atm)/ (mol x K)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 13QAP: Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant...

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For which reactions in Exercise 34 is Kp equal to K?
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Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant K1. (b) Write an equilibrium constant expression for the formation of one mole of B(g) and call the equilibrium constant K2. (c) Relate K1 and K2.
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
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The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
Phosgene, COCl2, used in the manufacture of polyurethane plastics, is prepared from CO and Cl2. CO(g)+Cl2(g)COCl2(g) An equilibrium mixture at 395C contains 0.012 mol CO and 0.025 mol Cl2 per liter, as well as COCl2 If Kc at 395C is 1.23 103, what is the concentration of COCl2?
In the contact process, sulfuric acid is manufactured by first oxidizing SO2 to SO3, which is then reacted with water The reaction of SO2 with O2 is 2SO2(g)+O22SO3(g) A 2.000-L flask was filled with 0.0400 mol SO2 and 0.0200 mol O2. At equilibrium at 900 K, the flask contained 0.0296 mol SO3 How many moles of each substance were in the flask at equilibrium?
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