D Question 7 This reaction, 2 NH3(g) N₂(g) + 3 H₂(g), is an exothermic reaction that is at equilibrium in a 20.00 L vessel with a movable piston on one side. Only answering in terms of LeChatelier's Principle (shift left, shift right, or no change), how will the reaction establish a new equilibrium when the following change is made? Change: decrease the volume of the vessel by moving the piston A. There is no change B. The reaction proceeds to the left C. The reaction proceeds to the right D. Not enough information OA OB OC OD

D Question 7 This reaction, 2 NH3(g) N₂(g) + 3 H₂(g), is an exothermic reaction that is at equilibrium in a 20.00 L vessel with a movable piston on one side. Only answering in terms of LeChatelier's Principle (shift left, shift right, or no change), how will the reaction establish a new equilibrium when the following change is made? Change: decrease the volume of the vessel by moving the piston A. There is no change B. The reaction proceeds to the left C. The reaction proceeds to the right D. Not enough information OA OB OC OD

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 6ALQ

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Similar questions

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.
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.
A piece of gold (10.0 g, CAu = 0.129 J/g K) is heated to 100.0 C. A piece of copper (also 10.0 g, CCu = 0.385 J/g K) is chilled in an ice bath to 0 C. Both pieces of metal are placed in a beaker containing 150. g H2O at 20 C. Will the temperature of the water be greater than or less than 20 C when thermal equilibrium is reached? Calculate the final temperature.
The following reaction occurs when a burner on a gas stove is lit: CH4+2O2(g)CO2(g)+2H2O(g) Is an equilibrium among CH4, O2, CO2, and H2O established under these conditions? Explain your answer.
. Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
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.
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?

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