Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) + Cl2(g) at 291 K given the following information,
2 N2(g) + 2 O2(g) ↔ 4 NO(g); K = 5.397×10-61
NO + 1/2 Cl2(g) ↔ NOCl(g); K = 2.432×104
Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) +...
Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) + Cl2(g) at 279 K 2 N2(g) + 2 O2(g) ↔ 4 NO(g); K = 6.503×10-62 NO + 1/2 Cl2(g) ↔ NOCl(g); K = 4.122×104
Given the values of K shown below, determine the value of K for the reaction, 2 NOCl <=> O2(g) + N2(g) + Cl2(g) 1/2 N2 + 1/2 O2(g) <=> NO(g) K = 0.0848 NO(g) + 1/2 Cl2(g) <=> NOCl(g) K = 0.0388 Give your answer to the nearest whole number
. Determine the value of the equilibrium constant for the reaction N2 (g) + 2O2 (g) ↔ N2O4 (g) from the following equations. ½ N2 (g) + ½ O2 (g) ↔ NO (g) KC = 6.9 x 10-16 2NO2 (g) ↔ 2NO (g) + O2 (g) KC = 4.5 x 10-13 2NO2 (g) ↔ N2O4 (g) KC = 6.7
A mixture of 0.1182 mol of O2, 0.05082 mol of NOCl, 0.1918 mol of NO2, and 0.1196 mol of Cl2 is placed in a 1.0-L steel pressure vessel at 604 K. The following equilibrium is established: 1 O2(g) + 2 NOCl(g) 2 NO2(g) + 1 Cl2(g) At equilibrium 0.03160 mol of NOCl is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of O2, NOCl, NO2, and Cl2. Peq(O2) = . Peq(NOCl) = . Peq(NO2) = . Peq(Cl2)...
consider following reaction: 2 NO + Cl2⇌ 2 NOCl for which K= 6.25*10^4. Calculate K for the following reaction 6 NOCl⇌ 6 NO + 3 Cl2
10 Use the following reactions and given ΔH values: 1/2 N2 (g) + 1/2 O2 (g) -> NO (g) ΔH = 90.3 kJ NO (g) + 1/2 Cl2 (g) -> NOCl (g) ΔH = -38.6 kJ Enter your answer with the appropriate significant figures and in terms of kJ. Do not include the unit in your answer.
ΔH is positive for the equilibrium N2 (g) + O2 (g) ↔ 2 NO (g). If we lower the temperature, (A) the equilibrium shifts to the left (more N2 + O2 gases formed) (B) the equilibrium shifts to the right (more NO gas formed) (C) Equilibrium does not shift because there are the same number of molecules on left side as on the right (D) Equilibrium does not shift because temperature does not affect the reaction rates why?
Calculate the activation energy for the gas phase reaction: 2 NOCl(g) ® 2 NO(g) + Cl2(g) given the following data: T(K) rate constant (L mol-1s-1) 400 6.95 × 10-4 450 1.98 × 10-2 500 2.92 × 10-1 550 2.60 600 16.3
Determine the value of the equilibrium constant, Kgoal, for the reaction N2(g)+H2O(g)⇌NO(g)+12N2H4(g), Kgoal=? by making use of the following information: 1. N2(g)+O2(g)⇌2NO(g), K1 = 4.10×10−31 2. N2(g)+2H2(g)⇌N2H4(g), K2 = 7.40×10−26 3. 2H2O(g)⇌2H2(g)+O2(g), K3 = 1.06×10−10 Express your answer numerically. Kgoal = Part B Determine the equilibrium constant, Kgoal, for the reaction 4PCl5(g)⇌P4(s)+10Cl2(g), Kgoal=? by making use of the following information: P4(s)+6Cl2(g)⇌4PCl3(g), K1=2.00×1019 PCl5(g)⇌PCl3(g)+Cl2(g), K2=1.13×10−2 Express your answer numerically. Kgoal =
At 500.0 K, gaseous NOCl decomposed to NO and Cl2 according the
following reaction:
2NOCl(g) ⇌ 2NO(g) + Cl2(g)
If 1.00 mole of NOCl is placed in a 1.00 liter contained, and at
equilibrium, the
concentration is 0.91M, what is the equilibrium constant,
Kc?
4. At 500.0 K, gaseous NOCI decomposed to NO and Cl2 according the following reaction: 2NOCI(g) = 2NO(g) + Cl2(g) If 1.00 mole of NOCI is placed in a 1.00 liter contained, and at equilibrium, the...