"Given the Kc of the first reaction below, find the Kc of the second reaction. A (g) + B (g) ⇌ AB (g) Kc = 9.517x10 2 2 A (g) + 2 B (g) ⇌ 2 AB (g) Kc = ?"
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"Given the Kc of the first reaction below, find the Kc of the second reaction.
A (g) + B (g) ⇌ AB (g) Kc = 9.517x10 2
2 A (g) + 2 B (g) ⇌ 2 AB (g) Kc = ?"
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- 3) Based on the information below, determine the value of the unknown equilibrium constant, Kc. 4 CO2 (g) + 2 H2O (g) « 4 O2 (g) + 2 CH2CO (g)Kc = 3.7 x 1017 CO2 (g) + 2 H2O (g) « CH4 (g) + 2 O2 (g)Kc = 8.3 x 10-15 CH4 (g) + CO2 (g) « CH2CO (g) + H2O (g)Kc = ?On the basis of Kc for the following reaction, would you expect the reaction to go almost completely to product at equilibrium? 2SO2(g) + O2(g) ↔ 2SO3(g); Kc = 3x1025 Yes No On the basis of Kc for the following reaction, would you expect nearly complete reaction at equilibrium? 2HF(g) ↔ 2H2(g) + F2(g); Kc = 3x10-95 Yes NoUse the data shown here to find the equilibrium constant (Kc) for the reaction, A(g) → 2 B(g) +C(g) A(g) +2 X(g) +C(g) B(g) → X(g) O 984 O 26.8 O 6.10 x 10-4 O 10 O 244x103 Kc = 1.55 Kc =25.2
- 11) Into a 1.00 liter flask is placed 0.822 moles of SO3. At equilibrium 36.7% of the SO3 has decomposed. What is the value of the equilibrium constant? 2 SO3 (g) « 2 SO2 (g) + O2 (g)Kc = ?Consider the following reaction: CO(g) + 3H2 (g) ⇌ CH4 (g) If Kc = 3.46 What is Kc for the following reaction? CH4 (g)⇌CO(g) + 3H2 (g)Given these reactions and their equilibrium constants, CO(g) + 3 H₂(g) → CH4(g) + H₂O(g) K = 3.93 N₂(g) + H₂(g) = NH3(g) Kc = 0.324 determine Ke for the following reaction. CO(g) + 2 NH3(g) CH4(g) + H₂O(g) + N₂(g) Your Answer: Kc = 37.4
- Consider the reaction: 2 NH3(g) N₂(g) + 3H₂(g). At T = 740 K, the equilibrium constant Kc for this reaction is Kc = 10. What is the correct form of the equilibrium constant Kc for this reaction? (A) Kc = [N₂] [H₂]³ (B) Kc (C) Kc = (D) Kc = (E) Kc - 2[NH3] [N₂]+3 [H₂] [N₂] +3 [H₂] 2[NH3] 2 [NH3] [N₂] [H₂] ³ 13 [N₂] [H₂] ³ [NH3]²2. Given the reaction: N2(g) + 3H2 (g) = 2NH3 (g) If Kc for this reaction is 4.5 x 10-4 at 400 K, what is the equilibrium constant KR at the same temperature?At 25 °C, the following reactions have the equilibrium constants noted to the right of their equations. 2CO(g) + O₂(g) ⇒ 2CO₂(g) Kç= 3.3 × 10⁹1 2H₂(g) + O₂(g) → 2H₂O(g) Kc= 9.1 × 108⁰ Use these data to calculate Kc for the reaction H₂O(g) + CO(g) ⇒ CO₂(g) + H₂(g) Kc= i
- Calculate Kc for the following equilibrium. Be sure to use the correct significant figures. 2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g) Kp = 2.5 x 10^10 at 425. KN2(g) + O2 (g) 2 NO that is run at 25 ̊C, Kc = 1×10-30. Calculate the equilibrium constant for the reaction:2 NO N2 (g) + O2(g)Consider the following equilibria: 2SO3(g) 2SO2(g) + O2(g) Kc1 = 2.3 × 10 – 7 2NO3(g) ⟷ 2NO2(g) + O2(g) Kc2 = 1.4 ×10 – 3 Calculate the equilibrium constant for the reaction: SO2(g) + NO3(g) ⟷ SO3(g) + NO2(g) A 1.3 × 10 – 2 B 1.6 × 10 – 4 C 78 D 6.1 × 103