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For the following equation at 500 K, Kc = 7.9 x 1011
.H2(g) + Br2(g) ⇌ 2 HBr(g)
Find the Kc values for the following equations:
a) 2 HBr(g) ⇌ H2(g) + Br2(g) Kc = ?
b) 4 HBr(g) ⇌ 2 H2(g) + 2 Br2(g) Kc = ?
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- The equilibrium constant for the reaction NO(g) + 1/2 O2(g) ⇌ NO2(g) has a value of Kc = 1.50 at a certain temperature. What is the value of Kc for the reaction 2 NO2(g) ⇌ 2 NO(g) + O2(g) ? (Write your answer with 2 significant numbers)Consider the following general reaction:2A(g) + 2B(g) ⇌ 3C(g) The reaction was measured to have an equilibrium reaction constant (K) of 0.0100 at 100 K. If the reaction has a standard enthalpy change (ΔHrxn) of 500.3 J/mol, what should the equilibrium reaction constant be when the temperature is 800 K? (Please provide your answer to 3 significant figures.)Benzene is one of the compounds used as octane enhancers in unleaded gasoline. It is manufactured by thecatalytic conversion of acetylene to benzene: 3C2 H2(g) ⇌ C6 H6(g). Which value of Kc would make this reactionmost useful commercially? Kc ≈ 0.01, Kc ≈ 1, or Kc ≈ 10. Explain your answer
- Calculate Kc for the following equilibrium: 2SO2(g) + O2(g) ⇌ 2SO3(g); Kp = 2.5 × 1010 at 625 K. Kc = × 10Calculate the value of Kc for the reaction: 2 NO(g) + Br2(g) ⇌ 2 NOBr (g) using the following information. Do NOT use scientific notation. 2 NO(g) ⇌ N2(g) + O2(g) Kc1 = 1 x 1030N2(g) + Br2(g) + O2(g) ⇌ 2 NOBr(g) Kc2 = 2 x 10-27Consider the following reactions: 2B(g) ⇌ B2(g) Kc=1.585 2B(g) + A2(g) ⇌ AB2(g) + C(g) Kc=1.610 AB2(g) ⇌ C(g) + B2(g) Kc=0.208 What is the value of the equilibrium constant for the following reaction? A2(g) + 2B2(g) ⇌ 2 AB2(g) Report your answer with three decimals. Enter numbers only; do not enter units.
- Determine the value of the equilibrium constant, Kgoal, for the reaction N2(g)+O2(g)+H2(g)⇌12N2H4(g)+NO2(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. 2NO(g)+O2(g)⇌2NO2(g), K3 = 6.00×10-13The value of Keq for the equilibrium N2 (g) + O2 (g) ⇌ 2 NO (g) is 4.2 × 10–31 at 27 °C. What is the value of Keq for the equilibrium below? 4 NO (g) ⇌ 2 N2 (g) + 2 O2 (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 following reactions: B2(g) ⇌ 2B(g) Kc=0.593 2B(g) + A2(g) ⇌ AB2(g) + C(g) Kc=8.528 C(g) + B2(g) ⇌ AB2(g) Kc=1.062 What is the value of the equilibrium constant for the following reaction? A2(g) + 2B2(g) ⇌ 2 AB2(g) Report your answer with three decimals.At a particular temperature, Kc = 6.0 × 102 for2NO(g) + 2H2(g) ⇌ N2(g) + 2H2O(g)Calculate Kc for each of the following reactions:(a) NO(g) + H2(g) ⇌ 12N2(g) + H2O(g) Kc = × 10(b) 2N2(g) + 4H2O(g) ⇌ 4NO(g) + 4H2(g)At a particular temperature, Kc = 6.0 × 102 for2NO(g) + 2H2(g) ⇌ N2(g) + 2H2O(g)Calculate Kc for each of the following reactions:(a) NO(g) + H2(g) ⇌ 12N2(g) + H2O(g)