1. For the reaction at 20°C, NH3(aq) + H+ (aq) = NH+ (aq) the equilibrium constant is calculated to be K = 4.5 × 108. a. Write the equilibrium expression for this reaction. b. From the size of the number for K, does the equilibrium lie to the left or to the right?

At a particular temperature, K = 3.68 for the reaction SO2(g) + NO2(g) = SO3(g) + NO(g) Calculate the concentrations of all four gases at equilibrium when 0.574 mol of each gas is mixed in a 1.000-L flask. (In other words, the concentration of each gas is 0.574 M.) HOW DO WE GET THERE? We will define the change in the concentrations to reach equilibrium in terms of x. Let x equal the number of moles per liter of SO, and NO, consumed to reach equilibrium. SO2(g) + NO2(g) = SO3(g) + NO(g) Initial: 0.574 0.574 0.574 0.574 Change: -X +x +x -x Equilibrium: 0.574-x 0.574-x 0.574+x 0.574+x Therefore, [SO,]]NO] [SO,]]NO,] (0.574+æ)(0.574+æ) (0.574 – x)(0.574 – x) K = 3.68 = What is the value of x? X =

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

5. At 100.0°C, the equilibrium constant K for the reaction C(s) + 1/2O2(g) CO(g) is 2.58 x 10°. Write an equilibrium constant expression for this reaction. What is the numerical value of the equilibrium constant for each of the following reactions: 2.58x10 a. CO(g) C(s) + 1/2O2(g) at 100.0°C b. 4C(s) + 2O2(g) 4CO(g) at 100.0°C c. C(s) + 1/2O2(g) CO(g) at 125.0°C 3 [co] = [0₂]

2 CO₂ (g) = 2 CO (g) + O₂ (g) 1. Write the K. expression for this balanced equation. 2. If, at equilibrium, the concentrations of the reactants and products are as follows: [CO] = 0.00025 M, [0₂] = 0.00050, [CO₂] = 0.25 M, calculate the value for Kc. 3. Where does the equilibrium lie, towards the products or reactants? How can you know?

Consider the reaction A + B C+D, which has an equilibrium constant, K, equal to 3.4 x 102. If one begins a reaction by placing 0.600 moles of A in a 1.0 L container as well as 0.150 moles of 1. B, what will be the equilibrium concentrations of A, B, C, and D? Write your answers in the spaces provided below. a. [А] b. [B]= [C]= С. d. [D]= Once the reaction in problem 1 reaches equilibrium, some additional B is injected into the flask 2. from an outside source. LeChatelier's principle says the reaction will (circle one): be unchanged shift to the right shift to the left Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L of 3. water, what will be the equilibrium concentrations of the species below: a. [Pyridine] = b. [Pyridine-H] (the pyridinium ion) [ОН-] 3 С. What is the pH of the solution in problem 4 (above)? .

At 773 °C, a mixture of CO(g), H2(g), and CH3OH(g) was allowed to come to equilibrium. The concentrations were determined to be: [CO] = 0.105 M, [H2] = 0.250 M, [CH3OH] = 0.00261 M. Calculate K. for the reaction CO(g) + 2H2(g) CH3OH(g) Kc = %3D

Consider this reaction which at a specified temperature has K =546.H +l(g) 2HI(g)If 0.25 M HI(g), 0.25 M H(g) and 0.25 M l(g) are placed in a vessel and the reaction attains equilibrium what is the ​[H] at equilibrium?