The equilibrium for the formation of dinitrogen tetraoxide gas (N,0.) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: 2 NO, (g) + N2O2 (g) What is the value of Kp at this same temperature? K = 1.7 x 1026 at 40,0°C (A) (B) (C) 4.4 x 10-25 6.6 x 1028 5.2 x 107 (D) 6.5 x 1030 (E) 5.9 x 1025

The equilibrium for the formation of dinitrogen tetraoxide gas (N,0.) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: 2 NO, (g) + N2O2 (g) What is the value of Kp at this same temperature? K = 1.7 x 1026 at 40,0°C (A) (B) (C) 4.4 x 10-25 6.6 x 1028 5.2 x 107 (D) 6.5 x 1030 (E) 5.9 x 1025

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

Predict the effect of increasing pressure for each of the following equilibriums: (a) 2H,0 (b) SIO2 (s) + N. 2H, e + 2NO (g) (g) 2 (g) 2 (g) + 4HF (g) SİF 4 (g) + 2H,0 (g) (с) СО + H, '2 (g) + Ca + H,0 (g) (g) (s) 2.
Equilibrium mixture in a 2.50 L flask at 250 °C in the reaction PCI3(g) + Cl₂(g) →PCI5(g); It contains 0.105 g PCI5, 0.220 g PCI3, and 2.12 g Cl₂. What is the value of (a) Kc and (b) Kp for this reaction at 250 °C? P: 31 g/mol; CI: 35.5 g/mol
4NH3(g) +50₂(g) = 4NO(g) + 6H₂O(g) AH = -1000. kJ K = 1.35 The equilibrium concentrations are [NH3] = 0.20M, [02] = 0.90M, [H2O] = 1.34 M, and [NO] = [?] What is the equilibrium concentration of NO at 25 °C? [NO] M Enter
The equilibrium constant, K, for the following reaction is 1.77x10 3 at 568 K. NH4CI(s) NH3(g) + HCI(g) Calculate Ke at this temperature for the following reaction: NH3(g) + HCl(g) NH4CI(s) Kc =
The following reaction takes place into a constant-volume flask at 427°C: CCL(g) = C(s) +2 C2(g) AH=132 kJ At 427°C, the equilibrium constant for the reaction given above is K. = 1.3×10-2. A flask is filled with 2.00 atm of CCl4 at 427°C. (a) What is the value of K for this reaction? (R=0.082 L.atm/mol.K) (b) What are the partial pressures of CClL, Ch and the total pressure at equilibrium? (c) How will the equilibrium pressure of CCl(g) change if the temperature is increased? (d) How will the equilibrium system respond if the volume of the flask is reduced?
11
For the equilibrium N2O4(g) <----> 2 NO2(g), at 298 K, Kp = 0.15. For this reaction system, it is found that the partial pressure of N2O4 is 3.7 × 10^–2 atm at equilibrium. What is the partial pressure of NO2 at equilibrium?
12.) A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g) = N2(g) + 3H2(g) At equilibrium, the mixture contained to following concentrations: [H2] = 0.0283 M, [N2] = 0.00944 M,[NH3] = 0.101 M. What is Kp at this temperature?
When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen. CO(g) + H2O(g) <--> CO2(g) + H2(g) +heat For each of the following changes at equilibrium, indicate whether the equilbrium shifts in the directions of the products, the reactants, or does not change: (a) decreasing the temperature (b) adding more H2(g) (c) removing some CO2(g) (d) adding more H2O(g) (e) decreasing the volume of the container
2) For the reaction, PCI:(g) = PCl:(g) + Ch(g) at 327°C, the equilibrium constant, Ke is 0.234. Suppose that 2.082 g PCIIS is placed in an evacuated 200 mL bulb, which is then heated to 327°C. (R = 0.082 L atm mol'K', PCIS = 208.2 g/mol) (a) What would be the pressure of PCIs if it did not dissociate? (b) What is the partial pressure of PCIS at equilibrium? (c) What is the total pressure in the bulb at equilibrium? (d) What is the fraction of PCIS at cquilibrium?
Please help with this
(b) At 100° C, the Keq for the Haber process is 4,51 X 10-5: N₂ + 3 H₂ 2 NH3 Consider the following reaction conditions and determine if the system is at equilibrium. If not, indicate the direction in which the reaction must proceed to establish equilibrium (i) PNH3 105 atm, PN2 = 35 atm and PH2 = 495 atm (ii) PNH3 35 atm, PN2 = 0 atm and PH2 = 595 atm (iii) PNH3 = 26 atm, PN2 = 202 atm and PH2 = 42 atm (iv) PNH3 105 atm, PN2 = 5 atm and PH2 = 55 atm