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Consider the equilibrium system: N2O4(g) + 2 NO2(g) for which Kp = 0.1134 at 25 °C...
Consider the following system at equilibrium: 2 NO2(g)⇄ N2O4(g) If 2.00 M NO2 is placed in a flask and allowed to react. At equilibrium, 1.80 M NO2 is present. A. Calculate the equilibrium concentration of N2O4. B. Calculate the equilibrium constant, K
15. Consider the reaction 2 NO2(g) N2O4(g) . (a) Using Gf N2O4(g) = 97.79 kJ/mol and Gf NO2(g) = 51.3 kJ/mol, calculate G° at 298 K. kJ (b) Calculate G at 298 K if the partial pressures of NO2 and N2O4 are 0.35 atm and 1.60 atm, respectively. kJ 16. Consider the reaction given below. H2(g) + F2(g) 2 HF(g) (a) Using thermodynamic data from the course website, calculate G° at 298 K. kJ (b) Calculate G at 298 K...
1) Kc = 45 for the equilibrium : 2 NO2(g) <====> N2O4 (g) at a temperature 85 C a) What is Kc for N2O42 <====> NO2(g) ? b) What is Kp for 2 NO2(g) <====> N2O4 (g) at 85 C? R= 0.0821 L-atm/ k-mol 2) The pH of seawater is 8.10 This corresponds to ________ M H+
Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.870 atm, and N2O4 at a pressure of 0.0757 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished?
Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.722 atm, and N2O4 at a pressure of 0.0521 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? PNO2= ?? atm PN2O4= ?? atm
Question text Calculate the equilibrium constants, KpKp and KcKc for the equilibrium reaction N2O4(g)⇄2NO2(g)N2O4(g)⇄2NO2(g) at 298 K. N2O4(g)N2O4(g) NO2(g)NO2(g) S0S0 (J/K/mol) 304.29 240.06 ΔfH0ΔfH0 (kJ/mol) 9.16 33.18 Select one or more: A. Kp=9.23Kp=9.23 , Kc=12.3Kc=12.3 B. Kp=0.563Kp=0.563 , Kc=0.33Kc=0.33 C. Kp=0.144Kp=0.144 , Kc=0.0058Kc=0.0058 D. Kp=0.355Kp=0.355 , Kc=1.23
At a particular temperature, Kp-0.39 for the reaction below. N204(g) 2 NO2(g) (a) A flask containing only N204 at an initial pressure of 4.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. N2O4 NO2 atm (b) A flask containing only NO2 at an initial pressure of 9.6 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. No2 (e) From your answers to parts (e) and (b), does it matter...
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
Consider the decomposition of N204(g) into NO2(g). N204(g) = 2 NO2(g) kp = 47.9 at 400 K Suppose that 1.00 atm of N204 decomposes and reaches equilibrium at 400 K. Determine the partial pressure of NO2 at equilibrium. 1.96 atm 0.922 atm 1.92 atm 0.960 atm 0.979 atm
1At a certain temperature, 659 K, Kp for the reaction, N2O4(g) <=> 2 NO2(g), is 5.4 x 10-69. Calculate the value of DGo in kJ for the reaction at 659 K. 2Given the values of So given below in J/mol K and the values of ΔHfo given in kJ/mol, calculate the value of ΔGo in kJ for the combustion of 1 mole of propane to form carbon dioxide and gaseous water at 298 K. S (C3H8(g)) = 271 S (O2(g))...