3. Consider the following reaction: NH,HS(s) NH3(g) + H,S(g) At a certain temperature, K.= 8.5 x 10, A reaction mixture at this temperature containing solid NH.NS has [NH] = 0.166 M and [H,S] = 0.166. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached? Calculation must be shown to support your answer. More solid

CO(g) + H₂O(g) ⇒ H₂(g) + CO₂(g) K = 7.3@823 K A closed 5.0 L container initially holds 3.0 moles CO and 6.0 moles H2O. Calculate the concentrations of each material at equilibrium. What is the equilibrium concentration of H₂O? [H₂O] = [?] M

Enter your answer in the provided box. In an analysis of the following reaction at 100°C, Br2(g) + Cl2(g) = 2BRCI(g) the equilibrium concentrations of the reactants were found to be [Br2] = 4.3 × 10 M and [Cl2] = 7.4 x 10 M. The equilibrium constant is K. = 7.1. Determine the value of [BrCI].

6. Hydrogen gas is finding more acceptance as an alternative fuel. It is produced along with carbon dioxide by the reaction of carbon monoxide and gaseous water at 915 K. At this temperature, the equilibrium constant (K.) is 1.56. If this reaction is started in a 4.00 L closed system flask with 0.450 mol of CO, 1.25 mol H2O, 1.15 mol CO2, and 3.50 mol H2, calculate the concentrations of all substances in the flask initially and at equilibrium. Put these values in the ICE table below. (Hint: you will need to use the quadratic formula.) CO Н20 CO2 H2 INITIAL CHANGE EQUILIBRIUM 0.1125 0.3125 0.2875 0.875 -X -X +X +x e these values in the table. d. Calculate the reaction quotient, Q. e. Express the direction of equilibrium shift as an algebraic expression. Complete the change row of the table. f. Substitute the algebraic expressions into the equilibrium expression and solve for the equilibrium concentrations. Place these values in the table.

1. Consider the following reaction at 500 K: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 This reaction is allowed to reach equilibrium, and then analyzed and found to contain the following concentrations: [O2] = 1.0 x 10-3 M [NO2] = 5.0 x 10-2 M. Determine the equilibrium concentration of NO (g).

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)? .

The equilibrium constant, kc, for the reaction below is 0.10 at 25°c. 2ICl(g)=Cl2(g)+I2(g) Find the equilibrium concentration for chlorine gas, Cl2(g), if the equilibrium concentrations of ICl(g) and I2(g) are known to be 0.50 M and 0.40 M respectively.

Consider the following equilibrium process at 686 degrees celsius. CO2 (g) + H2 (g) ---> CO (g) + H2O (g) The equilibrium concentrations of the reaction species are [CO]= 0.0510 M, [H2]= 0.0410 M, [CO2]= 0.0840 M, and [H2O]= 0.0390 M. a) alculate Kc for the reaction at 686 degrees celcius. Round your answer to 3 significant figures. b) If we add CO2 to increase its concentration to 0.420 M, what will the concentration of all the gases be when equilibrium is reestablished? [CO2]=  M.  Round your answer to 3 significant figures. c) [H2] =  M. Round your answer to 2 significant figures. d) [CO]=  M. Round your answer to 2 significant figures. e) [H2O]=  M.  Round your answer to 2 significatnt figures

For the reaction CO(g) + H2O(g) <-> CO2(g) + H2(g) K = 3.88 at a certain temperature. If at this temperature in a certain experiment the equilibrium concentrations are [H2] = 2.0 M, [CO2] = 1.8 M, and [H2O] = 0.26 M, calculate [CO].