9.Chemistry 106in a particular mixture of reactants and products are [PCI5]=0.500 M, [PCI3]=0.150 M and [Cl₂]=0.600 M.The reaction PCL5(g) = PCl3(g) + Cl₂(g) has a K.-0.573 at 500 K. If the initial concentrationsa. In which direction will the reaction proceed to reach equilibrium? (Show all your work)b. Draw an ICE table:3p 150so beendenwater, Incluprillod bris grilom, eixs oriljent undersaturated, natured. Show your answer is correct.W walvanhobiano (einiog 27) Itmotoculexcel evio piloooc. What are the concentrations of all products and reactant when the mixture reaches equilibrium?Show all your work (Include them in your ICE table)MOahog00.08vide all the5

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19. in a particular mixture of reactants and products are [PCIs]=0.500 M, [PC13]=0.150 M and [Cl₂]=0.600 M. The reaction PCl5(g) = PCl3(g) + Cl₂(g) has a K.=0.573 at 500 K. If the initial concentrations a. In which direction will the reaction proceed to reach equilibrium? (Show all your work) b. Draw an ICE table: tomiby 2m 150 Chemistry 106 d. Show your answer is correct. hyrndse boere novit habiend (einiog 873 17 prilliod bris gnitiom,alxs orit todel seselevius gnilobos wand c. What are the concentrations of all products and reactant when the mixture reaches equilibrium? Show all your work (Include them in your ICE table) pebe 5

19. in a particular mixture of reactants and products are [PCIs]=0.500 M, [PC13]=0.150 M and [Cl₂]=0.600 M. The reaction PCl5(g) = PCl3(g) + Cl₂(g) has a K.=0.573 at 500 K. If the initial concentrations a. In which direction will the reaction proceed to reach equilibrium? (Show all your work) b. Draw an ICE table: tomiby 2m 150 Chemistry 106 d. Show your answer is correct. hyrndse boere novit habiend (einiog 873 17 prilliod bris gnitiom,alxs orit todel seselevius gnilobos wand c. What are the concentrations of all products and reactant when the mixture reaches equilibrium? Show all your work (Include them in your ICE table) pebe 5

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4) At high temperatures nitrogen (N₂) and oxygen (O₂) will react to form NO. N₂(g) + O₂(g) 2 NO(g) The value for the equilibrium constant for reaction 4.1 is Kc = 2.7 x 10-¹7 at some temperature T. A system initially has [N₂] = 0.0800 M and [0₂] = 0.0500 M. There is no NO initially present in the system. Find the value for [NO] that will be present at equilibrium. (4.1)
1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-
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Consider the reaction. PCI, (g) = PCI, (g) + Cl,(g) K. = 0.0420 The concentrations of the products at equilibrium are [PC13] = 0.140 M and [Cl2] = 0.170 M. What is the concentration of the reactant, PCI5 , at equilibrium? [PC!5] = M
2
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. Given the following reaction: H2+ I2² 2HI If the equilibrium [HI] is 0.060 M and the equilibrium [b] is 0.90 M, what is the equilibrium [H2] if the K. is 0.40? 2. For the reaction 250zig) + Ozg) = 250xg), the concentrations at equilibrium are [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M. What is the value of the equilibrium constant, Kc?
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)? .
NA van wwwwwwww 1. For the reaction, 2 NO (g) + 2 H₂ (g) = following equilibrium concentrations: [NO]= 8.1 x 10-³ M [N2] = 0.053 M N₂ (g) + 2 H₂O (g), calculate Keq given the [H₂] = 4.1 x 10-5 M [H₂O]= 2.9 x 10-³ M 2. Given the reaction, UO2 (g) + 4 HF (g) = UF4 (g) + 2 H₂O (g), predict the effect each of the following will have on the equilibrium of the reaction (shift to the reactant side, the product side, or no shift). a. Uranium dioxide (UO2) is added. c. Water vapor is removed. b. Hydrogen fluoride (HF) reacts with the walls of the reaction vessel. - 3. At a certain temperature, Keq = 150 for the reaction being studied in today's lab. Use Equation (3) to calculate the concentrations of Fe³+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 105 M. Assume the equilibrium concentrations of Fe³+ and SCN are equal.
6. Write the equilibrium constant expression for the following reactions. a. CHa (8) + 20; (B) → CO; (B) + 2H;0 (g) b. 4 NH3 (g) + 302 (g) → 2N2 (g) + 6H;0 (g) c. C (s) + 2H2 (g) CH4 (g)
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