Use the equilibrium constants for the following reactions at 700 °C
2SO2(g) + O2(g) 2SO3(g) | K1 = 4.8 | |
2NO(g) + O2(g) 2NO2(g) | K2 = 16 | |
to determine the equilibrium constant for the following
reaction.
SO 3(
g) + NO( g) SO 2(
g) + NO 2( g)
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Use the equilibrium constants for the following reactions at 700 °C 2SO2(g) + O2(g) 2SO3(g) K1 =...
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
Given the equilibrium constants for the following reactions: 2H2(g) + O2(g) → 2H2O(g) K1 = 3.74 x 1026 H2(g) + Cl2(g) → 2HCl(g) K2 = 9.73 x 1012 calculate the equilibrium constant for the reaction below. 4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(g)
Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + O2(g) ** NO2(g) (2) 2NO2(g) + 2NO(g) + O2(g) B. Which one of the following is the correct relationship between the equilibrium constants Ki and K- K2 = 2/K K2 = (1/K1)2 K2=-K1/2 K2 = 1/(2K1) K2 - 1/(2K1)
The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) ⇌ 2NO(g) Kc = 4.3 × 10−25 2NO(g) + O2(g) ⇌ 2NO2(g) Kc = 6.4 × 109 Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 2O2(g) ⇌ 2NO2(g)
9. The equilibrium constants for the following reactions are K, and K2 as shown, 2NO (g) +02 (g)2NO2 (2) Ki 2S02 (g) + 02 (g)2SO3 (g) K2 the equilibrium constant for the reaction, NO2 (g)+ SO2 (g)sNO (g)+SO3 (g), is K2 c. a. K,K2 e. none of these 2 2K 14 10. The solubility product expression (Kip) for the dissolution of Group I salt KCI) in water is K+ ICI 11. A 7 L sample of a gas is confined...
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 7 × 103 at a certain temperature. If at equilibrium, [SO2] = 0.0451 M and [O2] = 0.078 M, what is the equilibrium [SO3]?
At 850 K, the equilibrium constant for the reaction 2SO2(g)+O2(g)↽−−⇀2SO3(g) is ?c=15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium.
The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) ⇌ 2NO(g) Kc = 4.3 × 10−25 2NO(g) + O2(g) ⇌ 2NO2(g) Kc = 6.4 × 109 Determine the values of the equilibrium constants for the following equations at the same temperature: (a) 4NO(g) ⇌ N2(g) + 2NO2(g) × 10 (b) 4NO2(g) ⇌ 2N2(g) + 4O2(g) × 10 (c) 2NO(g) + 2NO2(g) ⇌ 3O2(g) + 2N2(g) × 10
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1260 K? Kp= ?
The reaction 2SO2 (g) + O2 (g) ↔ 2SO3 (g) is exothermic and at equilibrium. Which of the following action will shift equilibrium left? A Lower environment temperature B Add O2 to the system C Add a catalyst to slow down the reaction D Add Ne gas to the equilibrium E Increase the volume of the reaction chamber