The following equilibrium pressures were observed at a certain temperature for the reaction N₂ (9) + 3H₂(g)2NH3(g) PNH, 4.8 x 10-2 atm = PN₂ = 9.6 x 10-¹ atm PH₂ = 2.3 × 10-3 atm Calculate the value for the equilibrium constant K, at this temperature. K₂ = Kp If PN₂ = 0.810 atm, PNHS = 0.0287 atm, and PH, = 0.00868 atm, does this represent a system at equilibrium? Submit Answer Retry Entire Group 9 more group attempts remaining

The following equilibrium pressures were observed at a certain temperature for the reaction N₂ (9) + 3H₂(g)2NH3(g) PNH, 4.8 x 10-2 atm = PN₂ = 9.6 x 10-¹ atm PH₂ = 2.3 × 10-3 atm Calculate the value for the equilibrium constant K, at this temperature. K₂ = Kp If PN₂ = 0.810 atm, PNHS = 0.0287 atm, and PH, = 0.00868 atm, does this represent a system at equilibrium? Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

At 1000 K, a sample of pure NO₂ gas decomposes: 2 2NO₂(g) = 2NO(g) + O₂(g) The equilibrium constant Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.41 atm at equilibrium. Part 1 of 2 What is the pressure of NO? Be sure your answer has the correct number of significant digits. Part 2 of 2 atm x10 atm X What is the pressure of NO₂? Be sure your answer has the correct number of significant digits. Ś x10
The equilibrium constant, Kp, for the following reaction is 5.40 at 346 K:COBr2(g) CO(g) + Br2(g)Calculate the equilibrium partial pressures of all species when COBr2(g) is introduced into an evacuated flask at a pressure of 0.767 atm at 346 K. PCOBr2 = atm PCO = atm PBr2 = atm
The equilibrium constant (Kc ) for the reaction: PCl3 + Cl2 <=> PCl5 equals 51 at 235°C. If 0.648 mol of phosphorus trichloride and 0.748 mol chlorine (Cl2) are added to a 9.00 L reaction vessel, what is the amount of moles of Cl2 at equilibrium in the mixture at 235°C?
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
Consider the reaction: 2 H2S (g) ⇋ 2 H2 (g) + S2 (g) Kp = 2.4 x 10 -4 at 1073 K If the initial pressure of hydrogen sulfide is 755 torr, what will be the equilibrium partial pressure of each gas?
● Nitrogen dioxide decomposes according to the rection: 2NO₂(g) → 2 NO(g) + O₂(g) where Kp = 4.48x 10-13. A pressure of 0.75 atm of NO₂ is introduced into a 1.00 L container and allowed to come to equilibrium. What are the equilibrium partial pressure of NO(g) and O₂(g)?
Consider the following equilibrium process at 686 degrees celsius. CO2 (g) + H2 (g) ---> CO (g) + H2O (g) The equilibrium concentrations of the reaction species are [CO]= 0.0510 M, [H2]= 0.0410 M, [CO2]= 0.0840 M, and [H2O]= 0.0390 M. a) alculate Kc for the reaction at 686 degrees celcius. Round your answer to 3 significant figures. b) If we add CO2 to increase its concentration to 0.420 M, what will the concentration of all the gases be when equilibrium is reestablished? [CO2]= M. Round your answer to 3 significant figures. c) [H2] = M. Round your answer to 2 significant figures. d) [CO]= M. Round your answer to 2 significant figures. e) [H2O]= M. Round your answer to 2 significatnt figures
At 2516 °C the equilibrium constant for the reaction: 2 BrCl(g) Br₂(g) + Cl₂(g) is Kp = 0.863. If the initial pressure of BrCl is 0.00277 atm, what are the equilibrium partial pressures of BrCl, Br₂, and Cl₂? p(BrCl) = p(Br₂) = p(Cl₂) =
60) The following are the values of the equilibrium constant, K, for four different chemical reaction systems. For each of the chemical reaction systems, describe the equilibrium position of the given temperature as mostly products, mostly reactants, or equal concentrations of reactants and products. a) K= 10-12 at 25 °C
3 A + 2 B → 1 CCalculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 6.87 M and [B] is 6.38 M. After the reaction has reached equilibrium, [C] is 1.47 M. Unfortunately, significant figures cannot be taken into account here, so please ignorethem this time.
What is the value of the equilibrium constant Kc of the reaction at the temperature of the vessel?
Consider the equilibrium system below. For this reaction, Kp = 205. If the equilibrium partial pressure of Cl2 is 0.050 atm and the partial pressure of NOCl is 0.095 M what is the equilibrium partial pressure of NO? 2 NO (g) + Cl2 (g) <-> 2 NOCl (g)