1. Sulfur trioxide decomposes spontaneously to form sulfur dioxide and oxygen gases according to the following balanced equation: 2SO, * 2SO, + O2 Under certain conditions, the equilibrium constant for the reaction is 6.9 x 10". What concentration of oxygen can be expected when 0.400 mol of SO, comes into equilibrium in a 2.00-L vessel? a. 360 b. Is this mixture at equilibrium? In a 1.00-L container is placed 0.10 mol ofO, 0.50 mol of SO, and 0.20 mol of SO, If not, predict in which direction the reaction will shift. An equilibrium mixture of the same three gases is combined with 0.10 mol of Ar reaction responds by producing more SO, с. The 3 Explain this new equilibrium shift. d. Describe how might a sulfur trioxide manufacturer try to minimize this decomposition reaction? Please choose a method different from part c.

1. Sulfur trioxide decomposes spontaneously to form sulfur dioxide and oxygen gases according to the following balanced equation: 2SO, * 2SO, + O2 Under certain conditions, the equilibrium constant for the reaction is 6.9 x 10". What concentration of oxygen can be expected when 0.400 mol of SO, comes into equilibrium in a 2.00-L vessel? a. 360 b. Is this mixture at equilibrium? In a 1.00-L container is placed 0.10 mol ofO, 0.50 mol of SO, and 0.20 mol of SO, If not, predict in which direction the reaction will shift. An equilibrium mixture of the same three gases is combined with 0.10 mol of Ar reaction responds by producing more SO, с. The 3 Explain this new equilibrium shift. d. Describe how might a sulfur trioxide manufacturer try to minimize this decomposition reaction? Please choose a method different from part c.

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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Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s)+3 H,0(g)→ Fe,O3(s)+3 H,(g) At a certain temperature, a chemist finds that a 9.2 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount ol. Fe 4.85 g Ar H,O 1.44 g Fe,O3 2.98 g H2 2.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 Ox10 Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
4. A. An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift"). a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.
Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H₂O(g) + H₂(g) + CO(g) Which of the following statements is/are CORRECT? 1. Increasing the concentration of H₂(g) will cause the reaction to proceed in the backward direction, increasing the equilibrium concentration of H₂O(g). 2. Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). 3. Increasing the amount of C(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). All statements are correct. 2 only 3 only 1 only 1 & 2 only
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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)? .
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