Lönsider the following reversible reaction equation: 2502(g) + 02(g) → 2S03(g) Ka = 1.2 x 10³ Complete the following sentences (a-e) by selecting the best choice from the dropdown menus. a) This is an example of a v equilibrium. b) At equilibrium, this system will contain mostly c) If more SO2 is added to this system at equilibrium, the reaction will shift towards the d) If oxygen gas is removed from this system at equilibrium, the reaction will shift towards the e) If the volume of this system at equilibrium is increased, the reaction will shift towards the

Lönsider the following reversible reaction equation: 2502(g) + 02(g) → 2S03(g) Ka = 1.2 x 10³ Complete the following sentences (a-e) by selecting the best choice from the dropdown menus. a) This is an example of a v equilibrium. b) At equilibrium, this system will contain mostly c) If more SO2 is added to this system at equilibrium, the reaction will shift towards the d) If oxygen gas is removed from this system at equilibrium, the reaction will shift towards the e) If the volume of this system at equilibrium is increased, the reaction will shift towards the

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 3RQ

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When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
Consider the reaction A+BC+D. A friend asks the following: “I know we have been told that if a mixture of A, B, C. and D is in equilibrium and more A is added, more C and D will form. But how can more C and D form if we do not add more B?” What do you tell your friend?
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
The following series of diagrams represent the reaction XY followed over a period of time. The X molecules are red and the Y molecules are green. At the end of the time period depicted, has the reaction system reached equilibrium? Justify your answer with a one-sentence explanation.
Summarize the steps for solving equilibrium problems (see the beginning of Section 12-6). In general, when solving an equilibrium problem, You should always set up an ICE table. What is an ICE table?
For the equilibrium 2 SO2(g) + O2(g) 2 SO3(g) Kc = 245 (at 1000 K) the equilibrium concentrations are [SO2] = 0.102, [O2] = 0.0132, and [SO3] = 0.184. The concentration of SO2 is suddenly doubled. Show that the forward reaction takes place to reach a new equilibrium.
. Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a closed vessel according to the equation H2O(g)+CO(g)H2(g)+CO2(g)a. You add more H2O to the flask. How does the new equilibrium concentration of each chemical compare to its origin al equilibrium concentration after equilibrium is re-established? Justify your answer. b. You add more H2to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
Equal amounts of two gases, A and B3, are placed in an evacuated container and react to form AB and B2. A(g)+B3(g)AB(g)+B2(g) The molecular scale diagram represents the relative amounts of each substance present once equilibrium is reached. Which of the following graphs best describes the progress of the reaction as it proceeds to equilibrium? Explain why the graph you chose must be the correct one.
For the reaction A2 + B2 2AB, diagram I depicts an initial reaction mixture, where A2 molecules are red and B2 molecules are green. Which of the diagrams II through IV is a possible equilibrium state for the reaction system? There may be more than one correct answer.
Antimony pentachloride decomposes according to this equation: SbCl5(g)SbCl3+Cl2(g) An equilibrium mixture in a 5.00-L flask at 443 C contains 3.85 g of SbCl5, 9.14 g of SbCl3, and 2.84 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00-L flask at the same temperature?
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.

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