By how much had the concentrations changed when the reaction reached equilibrium? The concentration of PCI3 has decreased by i M The concentration of Cl2 has decreased by i M The concentration of PCI5 has increased by i M What were the equilibrium concentrations? The equilibrium concentration of PCI3 = i M The equilibrium concentration of Cl2 = i M The equilibrium concentration of PCI5 = i M %3D What is the value of K. for this reaction at this temperature? Kc = i

Consider the following system at equilibrium: N₂(g) + 3H₂(g) = 2NH3(g); AH = 92.94 kJ Which of the following changes will shift the equilibrium to the right? Lincreasing the temperature II.decreasing the temperature III increasing the volume IV.decreasing the volume Vremoving some NH3 VLadding some NH3 VII removing some N₂ VIII. adding some N₂ O II, III, V, VIII O I, III, V, VII OI, VI, VIII OLIV, V, VIII O II, IV, V, VIII

c. HF & HCIO4 d. HBr & LIOH e. CH3COOH & KOH A sealed 1.00L flask is charged with 0.500 mol of I, and 0.500 mol of Br2. An equilibrium reaction ensues: 12 (g) + Br2 (g) =2 IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K is Select one: O a. K= 6.10 O b. K = 2.82 OC K = 882 Od. K= 110 Oe K= 131 en 13 The heat capacity of silver (Ag. 107.9 g maol), is 0.232 J g'K Calculate the energy needed to heat 2e mo saved II

Consider the following reaction at equilibrium.  Which of the following changes will shift the equilibrium to the left? CH4(g) + Cl2(g) ⇌  CCl4(l) + HCl(g)     ΔH°= –398 kJ I. Increasing the temperature II. Decreasing the temperature III. Increasing the volume IV. Decreasing the volume V. Removing some Cl2 VI. Adding some Cl2 VII. Removing some HCl VIII. Adding some HCl A. I, IV, VI, VII B. II, III, VI, VIII C. I, VI, VIII D. I, III, V, VIII E. II, IV, VI, VII

The chemical equation represents a reaction at equilibrium. 2SO3(g) = 2SO2 (g) +O2(g) Which of these shows the equilibrium constant expression for this chemical equation? A [O2][SO2]2/[SO3]2 B [O2]2[SO2]/2[SO3] C 2[SO3]/[O2]2[SO2] D [SO3]2/[O2][SO2]2

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).

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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)? .

Consider the reaction. PCI, (g) = PCI, (g) + Cl,(g) Ke = 0.0420 The concentrations of the products at equilibrium are [PC13] = 0.100 M and [Cl2] = 0.260 M. What is the concentration of the reactant, PCI5, at equilibrium? [PCI5] = M

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