5. This reaction has been allowed to reach equilibrium, 2 NH, (g) = N₂ (g) + 3 H₂ (g) Then additional H₂ is added. The reaction is allowed to reach a new equilibrium. Which statement is true about the new equilibrium compared to the first equilibrium? (A) [N₂] & [H₂] are both down, while [NH3] is up (B) [N₂] is up, [H₂] is down, while (NH3) is up (C) [N₂] & [H₂] are both up, while [NH3] is down (D) [N₂] is down, [H₂] is up, while [NH3] is up (E) None of these is correct You could add N₂ or NH

5. This reaction has been allowed to reach equilibrium, 2 NH, (g) = N₂ (g) + 3 H₂ (g) Then additional H₂ is added. The reaction is allowed to reach a new equilibrium. Which statement is true about the new equilibrium compared to the first equilibrium? (A) [N₂] & [H₂] are both down, while [NH3] is up (B) [N₂] is up, [H₂] is down, while (NH3) is up (C) [N₂] & [H₂] are both up, while [NH3] is down (D) [N₂] is down, [H₂] is up, while [NH3] is up (E) None of these is correct You could add N₂ or NH

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 10ALQ: . Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a...

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Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
. 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.
7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
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.
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