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Chemistry
- On the basis of the value of Kc decide whether or not you expect nearly complete reaction at equilibrium for each of the following: a N2(g)+O2(g)2NO(g);Kc=4.61031 b C2H4(g)+H2(g)C2H5(g);Kc=1.31021arrow_forward5. Dinitrogen pentoxide is added to an evacuated rigid container at 25°C. Given that the initial pressure is 1.00 atm and at equi- librium the pressure is 0.500 atm, determine the final pressure in the reaction vessel at equilibrium. 2N2O5(g) = 4NO2(g) + O2(8) (A) 0.750 atm (B) 1.00 atm (C) 1.25 atm (D) 1.75 atmarrow_forwardAn equilibrium mixture at a certain temperature contains 1.15 M N2, 1.35 M H2, and 0.415 M NH3 at 500 oC. What is the equilibrium constant Kc for the following reaction? NH3(g) + 3H2(g) ⇌ 2NH3(g) (A) Kc = 0.00902 (B) Kc = 0.0109 (C) Kc = 0.0609 (D) Kc = 0.178arrow_forward
- pts eoch) The equilibrium for the formation of dinitrogen tetraoxide gas (N,0.) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: 2 NO, (g) + N2O4 (g) What is the value of Kpat this same temperature? K = 1.7 x 1026 at 40.0°C (A) (B) (C) (D) (E) 4.4 x 10-25 6.6 x 10-28 5.2 x 1027 6.5 x 10-30 5.9 x 1025arrow_forwardThe equilibrium for the formation of dinitrogen tetraoxide gas (N204) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: K. = 1.7 x 10-26 at 40.0°C 2 NO2 (g) <→ N2O4 (g) What is the value of Kp at this same temperature? -25 (A) 4.4 x 10 (B) 6.6 x 10-28 (C) 5.2 x 10-27 (D) 6.5 x 10-30 (E) 5.9 x 1025arrow_forward9. The equilibrium constant for the reaction 2 BrCl (g) → Br2 (g) + Cl2 (g) at 25°C is Keq = 0.0172. What is the equilibrium constant for the reaction Br2 (g) + Cl2 (g) →2 BrCl (g)? (а) -0.0172 (b) 0.131 (c) 7.62 (d) 58.1 (e) none of thesearrow_forward
- A flask is charged with 1.540 atm of N2O4(g) and 0.97 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.N2O4(g) 2NO2(g)After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4? atm(b) Calculate the value of Kp for the reaction. (c) Is there sufficient information to calculate Kcfor the reaction? No, because the value of Kc can be determined experimentally only.Yes, because the partial pressures of all the reactants and products are specified. Yes, because the temperature is specified. If Kc can be calculated, find the value of Kc. Otherwise, enter 0.arrow_forward- The following reaction takes place into a constant-volume flask at 427°C:CCl4(g) ⇌ C(s) + 2 Cl2(g) ΔH=132 kJAt 427°C, the equilibrium constant for the reaction given above is Kc = 1.3×10-2. A flask isfilled with 2.00 atm of CCl4 at 427°C.(a) What is the value of Kp for this reaction? (R=0.082 L.atm/mol.K)(b) What are the partial pressures of CCl4, Cl2 and the total pressure at equilibrium?(c) How will the equilibrium pressure of CCl4(g) change if the temperature is increased?(d) How will the equilibrium system respond if the volume of the flask is reduced?arrow_forwardA flask is charged with 1.600 atm of N2O4(g) and 1.06 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.N2O4(g) 2NO2(g)After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4? atm(b) Calculate the value of Kp for the reaction. (c) Is there sufficient information to calculate Kcfor the reaction? Yes, because the partial pressures of all the reactants and products are specified. No, because the value of Kc can be determined experimentally only. Yes, because the temperature is specified. If Kc can be calculated, find the value of Kc. Otherwise, enter 0.arrow_forward
- The equilibrium constant for the following reaction is 260 at -1 °C. 2 NO(g) + Br₂(g) 2 NOBr(g) K 260 at -1 °C - Calculate the equilibrium constant for the following reactions at -1 °C. (a) 2 NOBr(g) (b) NOBr(g) ? 2 NO(g) + Br₂(g) NO(g) + 1/2 Br₂(g) K = K =arrow_forwardThe reaction N₂O4(g) 2NO₂(g) has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N₂O4 was 0.344 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO₂ = atm (b) What was the total pressure of the mixture of gases? total pressure = atmarrow_forwardA chemical equilibrium A ⇄ 2B has a forward rate constant, kf = 12 M –1 s–1, and a reverse rate constant, kr = 18 s–1. If the system has a concentration of [A] = 0.15 M at equilibrium, what is the concentration of B at equilibrium? (no scientific notation)arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning