The equilibrium constant for the reaction 2 HF (g) ⇌ H₂ (g) + F₂ (g) is 0.360 at a particular temperature. What is the equilibrium constant for the equation ½ H₂ (g) + ½ F₂ (g) ⇌ HF (g)? ANswer _____
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- Need ayuda:((( Part 1. What is the value for K if the equilibrium pressures for hydrogen, oxygen, and water are 1,0.5,1atm? What was calculated in part 1? A. K B. K subscript p C. K subscript C Part 3. Convert answer in part 1 to other K using the following equation. Assume reaction is performed at 25 Celsius. Round to first decimal place Kp=Kc (RT)^delta nThe following system was set up and allowed to come to equilibrium: C2H2(g) + 2 H2(g) ⇌ C2H6(g) At equilibrium, the concentration of ethyne was 0.210 mol/L, the concentration of hydrogen gas was 0.830 mol/L. The value of the equilibrium constant for the reaction at that temperature is 8. 10. What was the concentration of the ethane in mol/L? Answer in mol/L to 3 decimal places.Answer the following questions. Write the expression for the equilibrium constant for the reaction represented by the equation Na+(aq)+Cl−(aq)⇌NaCl(s). Is Kc > 1, < 1, or ≈ 1? Explain your answer. Write the expression for the equilibrium constant for the reaction represented by the equation PbCl2(s)⇌Pb2+(aq)+2Cl−(aq). Is Kc > 1, < 1, or ≈ 1? Explain your answer.
- Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), K1 = 9.11×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), K2 = 1.46×10−19, what is the equilibrium constant Kfinal for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq) Enter your answer numerically.Pick the correct equilibrium expression for the following reaction. 2 SO2(g) + 2 H2O(g) ↔ 2 H2S(g) + 3 O2(g)The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H2(g) + Br2(g) ⇌ 2HBr(g) Kc = 3.8 × 104 2HBr(g) ⇌ H2(g) + Br2(g) Kc = ? I don't understand how to get the kc? My answer is a decimal. I cannot figure this one out. Please help if able. Thanks.
- Calculate the value of [N 2] eq if [H 2] eq = 2.0 M, [NH 3] eq = 0.5 M, and K c = 2. N 2(g) + 3 H 2(g) --> 2 NH 3(g) 0.016 M 0.062 M 0.40 M 0.031 M 62.5 M2NO2 (?) ⇌ N2O4 (?) If there are 0.400 moles of N2O4 and 0.500 moles of NO2 in a 1.00 L flask at equilibrium at 20°C, what is the Keq?For the reaction: 2NOCl(g) ⟷⟷ 2NO(g) + Cl2(g) If the reaction were allowed to reach equilibrium and you were to remove some Cl2(g), what would happen? [Check all that are correct.] Group of answer choices - Equilibrium would shift to the right. - Equilibrium would shift to the left. - The amount of NOCl(g) would increase. - The amount of NO(g) would increase.
- Given the following information: 2 A(g) + B(g) ⇌ A2B(g) K1 = 5.0 x 104 2 A(g) + C2(g) ⇌ 2 AC(g) K2 = 3.2 x 103 What is the net equilibrium constant (Knet) for the reaction? 2AC(g) + 4A(g) + 3B(g) ⇌ 3 A2B(g) + C2(g)The Keq for the equilibrium below is 7.44 × 10-2 at 480.0 °C. 2 Cl2 (g) + 2 H2O (g) → 4HCl(g) + O2 (g) What is the value of Keq at this temperature for the following reaction? 2 HCl (g) + ½ O2 (g) →Cl2 (g) + H2O (g)QUESTION 6 The value of the equilibrium constant for the following reaction is 24 at a given temperature: N2(g) + 3H2(g) ⇌ 2NH3(g) If [N2] = 10.0 M, [H2] = 10.0 M, and [NH3] = 10.0 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium? Since Q = 0.01, the reaction is not at equilibrium, it will shift to the left. It is not possible to tell if the reaction is at equilibrium. Since Q = 1, the reaction is not at equilibrium, it will shift to the left. Since Q = 1, the reaction is not at equilibrium, it will shift to the right. Since Q = 100, the reaction is not at equilibrium, it will shift to the right. Since Q = 100, the reaction is not at equilibrium, it will shift to the left. The reaction is at equilibrium. To reach equilibrium, the value of Keq must change. Since Q = 0.01, the reaction is not at equilibrium, it will shift…