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3. The value of the equilibrium constant (Kc) for the reaction N₂(g) + 3H₂(g) = 2NH3(g) is 4.34x10 at 300 °C. Which of the following statements will be true regarding the system at equilibrium? a. The products will predominate. b. The reactants will predominate. c. Only reactants will be present. d. Only products will be present. e. Roughly equal amounts of products and reactants will be present.

3. The value of the equilibrium constant (Kc) for the reaction N₂(g) + 3H₂(g) = 2NH3(g) is 4.34x10 at 300 °C. Which of the following statements will be true regarding the system at equilibrium? a. The products will predominate. b. The reactants will predominate. c. Only reactants will be present. d. Only products will be present. e. Roughly equal amounts of products and reactants will be present.

Chemistry
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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Question 3 please. It's a practice exam. Will post the answer with it.
Answer Section MULTIPLE CHOICE 1. 2. 3. 4. 5. 6. 7. ANS: A 8. ANS: E 9. ANS: B 10. ANS: D 11. ANS: B ANS: E ANS: E ANS: B ANS: A ANS: D ANS: B 12. ANS: E 13. ANS: A 14. ANS: A 15. ANS: A 16. ANS: D 17. ANS: A 18. ANS: E 19. ANS: B 20. ANS: B 21. 22. ANS: A ANS: C
Transcribed Image Text:Answer Section MULTIPLE CHOICE 1. 2. 3. 4. 5. 6. 7. ANS: A 8. ANS: E 9. ANS: B 10. ANS: D 11. ANS: B ANS: E ANS: E ANS: B ANS: A ANS: D ANS: B 12. ANS: E 13. ANS: A 14. ANS: A 15. ANS: A 16. ANS: D 17. ANS: A 18. ANS: E 19. ANS: B 20. ANS: B 21. 22. ANS: A ANS: C
2. For the reaction 2HCl(g) = H₂(g) + Cl₂(g), Kc = 0.290 at 400 K. If 1.50x10³ M of HC1, H₂, and Ch₂ are mixed initially at 400 K, which one of the following will happen? The concentrations of HCl and Cl₂ will increase as the system approaches equilibrium. The concentrations of H₂ and Cl₂ will increase as the system approaches equilibrium. a. b. C. d. e. The system is at equilibrium. The concentrations of H₂ and HCI will decrease as the system approaches equilibrium. The concentration of HCI will increase as the system approaches equilibrium. 3. The value of the equilibrium constant (Kc) for the reaction N₂(g) + 3H₂(g) + 2NH3(g) is 4.34x10³ at 300 °C. Which of the following statements will be true regarding the system at equilibrium? a. The products will predominate. b. The reactants will predominate. c. Only reactants will be present. d. Only products will be present. e. Roughly equal amounts of products and reactants will be present. . A 3.80 mol sample of HI is placed in a 1.00 L vessel at 460 °C, which is allowed to undergo decomposition according to the equation 2HI(g) = H₂(g) + I₂(g). At equilibrium, there is 1.85 mol of I2(g) present in the flask What is the value of the equilibrium constant (Kc) for the reaction at 460 °C? 34.23 e. 4.22
Transcribed Image Text:2. For the reaction 2HCl(g) = H₂(g) + Cl₂(g), Kc = 0.290 at 400 K. If 1.50x10³ M of HC1, H₂, and Ch₂ are mixed initially at 400 K, which one of the following will happen? The concentrations of HCl and Cl₂ will increase as the system approaches equilibrium. The concentrations of H₂ and Cl₂ will increase as the system approaches equilibrium. a. b. C. d. e. The system is at equilibrium. The concentrations of H₂ and HCI will decrease as the system approaches equilibrium. The concentration of HCI will increase as the system approaches equilibrium. 3. The value of the equilibrium constant (Kc) for the reaction N₂(g) + 3H₂(g) + 2NH3(g) is 4.34x10³ at 300 °C. Which of the following statements will be true regarding the system at equilibrium? a. The products will predominate. b. The reactants will predominate. c. Only reactants will be present. d. Only products will be present. e. Roughly equal amounts of products and reactants will be present. . A 3.80 mol sample of HI is placed in a 1.00 L vessel at 460 °C, which is allowed to undergo decomposition according to the equation 2HI(g) = H₂(g) + I₂(g). At equilibrium, there is 1.85 mol of I2(g) present in the flask What is the value of the equilibrium constant (Kc) for the reaction at 460 °C? 34.23 e. 4.22
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