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 following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) ⇌...
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)
The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) Ke = 4.3 x 10-25 2NO(g) + O2(g) + 2NO:(8) K-6.4 x 10 Determine the values of the equilibrium constants for the following equations at the same temperature: (a) 4NO(g) = N2(g) + 2NO:(g) x 10 (b) 4NO:() = 2N:(0) + 40:(8) x 10 (c) 2NO(g) + 2NO3(g) = 30:(g) + 2N:(g) x 10
The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) Ke = 4.3 x 10-25 2NO(g) + O2(g) + 2NO:(8) K-6.4 x 10 Determine the values of the equilibrium constants for the following equations at the same temperature: (a) 4NO(g) = N2(g) + 2NO:(g) x 10 (b) 4NO:() = 2N:(0) + 40:(8) x 10 (c) 2NO(g) + 2NO3(g) = 30:(g) + 2N:(g) x 10
. 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
For the reaction N2(g) + O2(g) 2NO(g), Kc = 4.0 at a particular temperature. In a 1.0-L container, 1.0 mol of N2 and O2 are mixed. Determine the concentration of NO once equilibrium is reached at the given temperature. =________ Please explain so I understand
9. At a particular temperature, the following reactions have the equilibrium constants shown: S(s) + O2(g) = SO2(g) K-4.2 1052 2 S(s) + 3 02(g) = 2 SO3(g) K2 = 9.8* 10128 Calculate the equilibrium constant K; for the following reaction at the same temperature. 2 SO2(g) + O2(g) = 2 SO3(g) K; =
Calculate the change of enthalpy for the reaction N2 + O2 --> 2NO from the following reactions: Reaction 1: 4NH3 + 3O2 --> 2N2 + 6H2O Change in enthalpy: -1530 kJReaction 2: 4NH3 + 5O2 --> 4NO + 6H2O Change in enthalpy: -1170 kJReaction 3: 2N2 + 6H2O --> 4NH3 + 3O2 Change in enthalpy: +1530 kJ
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)
5.84 for which of the following reactions does delta H degree run represent an enthalpy of formation? A) 2N2(g) + 3O2(g) —-> 2NO(g) + 2NO(g) B) N2(g) + O2(g) —> 2NO (g) C) 2NO2(g) —> N2O4(g) D) N2(g) + 2O2(g) —> 2NO2 (g)
Given the following reactions N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ 2NO( g) + O2 (g) → 2NO2 (g) ΔH = -113.1 kJ the enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen 2NO2 (g) → N2 (g) + 2O2 (g) is ________ kJ.