1. Solid ammonium iodide decomposes to ammonia and hydrogen iodide gases at sufficiently high temperature. NH. w → NH3 + HI The equilibrium constant for the decomposition at 673K is 0.215. Fifteen grams of ammonium iodide is sealed in a 5.0 L flask and heated to 673K a. What is the total pressure in the flask b. How many grams of NHal decomposed

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.

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)? .

20.

7. Phosgene COCl2 is prepared from CO and Cl₂ CO (g) + Cl₂(g) COC1₂(g) An equilibrium mixture at 395 °C contains 0.012 mol CO and 0.025 mol Cl₂ per liter. If Kc at 395 °C is 1.23 X 10³, what is the concentration of COC1₂?

The equilibrium constant, K. , for the following reaction is 7.00x105 at 673 K. NH,I(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 6.89 L container at 673 K contains 2.67 mol of NH,I(s) and 0.210 mol of NH3, the number of moles of HI present is moles.

Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. = 1.80 at 250 °C A 0.3668 mol sample of PCI, (g) is injected into an empty 4.30 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCI, (g) at equilibrium. [PCl,] = M [PCI,] = M