At T 5 100°C the reaction SO2C-2(g) uv SO2-(g) Cl2(g) has an equilibrium constant K= 2.4. (a) Suppose the initial partial pressure of SO2Cl2 is 1.20 atm, and PSO2 = PCl2 = 0. Calculate the reaction quotient Q and state whether the reaction proceeds to the right or to the left as equilibrium is approached. (b) Calculate the partial pressures at equilibrium. (c) If the volume of the system is then decreased, will there be net formation or net dissociation of SO2Cl2

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.

The reaction: 2SO₂(g) + O₂(g) = 2SO3(g) has an equilibrium constant, Kc = 4.4 Suppose a mixture contains 0.22 M SO₂, 0.16 M O2, and 0.25 M SO3. Calculate the value of Qc and predict whether the system is at equilibrium or not at equilibrium. If not at equilibrium, indicate the direction of net reaction. (A) Qc = 0.12; system is not at equilibrium; a net forward reaction occurs to form more SO3 (B) Qc = 7.1; system is not at equilibrium; a net forward reaction occurs to form more SO3 (C) Q = 8.1; system is not at equilibrium; a net back reaction occurs to form more SO₂ and 0₂ (D) Qc = 4.4; system is at equilibrium and there is no net reaction

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)

At 25°C, the equilibrium constant for the reaction Blg) + Clg) 2A(3) is K,-0.0735.If the three gases are mixed in a rigid container having partial pressuros of 3.35, 185 and 0.693 atm for A, B and C, respectively, is the system at equilibrium? The system is at equilibrium. The reverse reaction must proceed to establish equilibrium. The volume of the container must be known to answer the question. The concentrations of all substances must be known to answer the question. The forward reaction must praceed to establish equilibrium,

For the following equilibrium system, K = 2.06×10 at 298K. HSO3 (aq) + HCIO(aq) H,S03(aq) + CIO (aq) Assuming that you start with equal concentrations of HSO, and HCIO , and that no H,SO, or CIO is initially present, which of the following best describes the equilibrium system? Appreciable quantities of all species are present at equilibrium. The forward reaction is favored at equilibrium. The reverse reaction is favored at equilibrium.

(5b) Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3 )2 as (P NH3)2. If either the numerator or denominator is 1, please enter 1   2 CuCl2(s)   ↔   2 CuCl(s) + Cl2(g)           K   =     (8c) Consider the following reaction where Kc = 6.50×10-3 at 298 K: 2 NOBr (g) 2 NO (g) + Br2 (g) A reaction mixture was found to contain 9.96×10-2 moles of NOBr (g), 4.61×10-2 moles of NO (g), and 4.42×10-2 moles of Br2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed .2. In order to reach equilibrium Kc must decrease .3. In order to reach equilibrium NO must be produced .4. Qc is less than Kc.5. The reaction is at equilibrium. No further reaction will occur.

The equilibrium constant Kc for the reaction,I2(g) + Br2(g) <-----> 2 IBr(g)is 314.7 at 425 K. What is the value of Kc for the equilibrium,1/2 I2(g) + 1/2 Br2(g) <-----> IBr(g)at 425 K?

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