The following reaction has an equilibrium constant, Kc, of 2.10 x 102  at a particular temperature:  N2 (g) + 3 H2 (g) → 2 NH3 (g) + You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, and the concentration of NH3 is 0.85 M. (a) Calculate the value of the reaction quotient Q. (b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed to reach equilibrium.

Consider the reaction 2 NH, (g) - N2 (g) + 3 H, (g) Starting with pure NH, at 700 K, a fraction a dissociates and the total pressure at equilibrium is 10 Ра. (i) Find the equilibrium constant K in terms of a. (i) The container is expanded and the total pressure drops. Qualitatively, explain briefly if you expect the following quantities to decrease, stay the same, or increase: (a) K (b) a.

The equilibrium constant for the reaction H2(g) + I½(s) = 2 HI(g) at 25°C is K = 0.345. (a) If the partial pressure of hydrogen is P1, = 1.00 atm and solid iodine is present, what is the equilibrium partial pressure of hydrogen iodide, PH1, at 25°C? (b) An excess of solid I, is added to a container filled with hydrogen at 25°C and a pressure of 4.00 atm. Calcu- late the pressures of H2(g) and HI(g) reached at equilibrium.

Consider the reaction: 2 NH3(g) = N₂(g) + 3 H₂(g). At T = 740 K, the equilibrium constant K for this reaction is K₂ = 10. 22. What is the correct form of the equilibrium constant K for this reaction? (A) Kc = (B) Kc = (C) Kc = 2[NH3] [N₂] + 3[H₂] (D) Kc = (E) Kc = [N₂][H₂]³ [N₂] + 3[H₂] 2[NH3] [NH3]² [N₂] [H₂] 3³ 3 [N₂] [H₂]³ 2 [NH3]²

2. Consider the following equilibrium: C (s) + H,O (g) = CÓ (g) + H, (g), AH® = +131.3 kJ-mol·' (1) Please write the expression of reaction quotient K. (2) Use Le Chatelier's Principle to state and explain the effect on the equilibrium when: (a) the pressure of H2O is increased; (b) the temperature is increased; (c) the concentration of the H, is increased; (d) The total pressure is increased by decreasing the volume. 作答

At 25.0 °C, the reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) is at equilibrium when PCO2 = 3.50 mbar, [H2O] = 55.5 mol L-1, [H+] = 39.8 µmol L-1, and [HCO3-] = 1.28 mmol L-1. Then an additional 4.00 mbar of CO2 is added to the system. Calculate ΔGrxn in kJ mol-1. (R = 8.3145 J mol-1 K-1)

Cyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5 H9 CH3) but with a different molecular structure. Cyclohexane Methylcyclopentane The equilibrium constant has been estimated to be 0.12 at 25 °C. If you had originally placed 0.053 mol of cyclohexane in a 2.8 L flask, what would be the concentrations of cyclohexane and methylcyclopentane when equilibrium is established? [cyclohexane] = M [methylcyclopentane] = M

An experimenter places the following concentrations of gases in a closed container: NOB1] = 0.475 M, [NO] = 2.59 x 10-2 M, Bra] = 5.57 x 10-2 M. These gases then react: 2NOB1(g) = 2NO(g) + Br2 (g) At the temperature of the reaction, the equilibrium constant Ke is 3.15 x 10-4. Calculate the reaction quotient, Qe, from the initial concentrations and determine whether the concentration of NOBr increases or decreases as the reaction approaches equilibrium. Qc = The concentration of NOBr decreases v

The equilibrium constant, Kc, for the following reaction is 0.0180 at 698 K. 2HI(g) ⇒ H₂(g) + 1₂ (9) Calculate the equilibrium concentrations of reactant and products when 0.293 moles of HI(g) are introduced into a 1.00 L vessel at 698 K. [HI] = [H₂] [1₂] = = ΣΣΣ

The equilibrium constant for the reaction 2 HF (g) H2 (g) + F2 (g) is 0.450 at a particular temperature. What is the equilibrium constant for the equation ½ H2 (g) + ½ F2 (g) HF (g)?