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nanging the temperature. 916040 =H₂(g) + Cl₂(g), Kc = 0.290 at 400 K. If 1.50x10³ M of HCL, H₂, and Cl₂ are mixed me of the following will happen? HCl and Cl₂ will increase as the system approaches equilibrium. H₂ and Cl₂ will increase as the system approaches equilibrium. brium. H₂ and HCI will decrease as the system approaches equilibrium. HCI will increase as the system approaches equilibrium. m constant (Kc) for the reaction N₂(g) + 3H₂(g) = 2NH3(g) is 4.34x10³ at 300 °C. ements will be true regarding the system at equilibrium? minate. minate. resent. resent. of products and reactants will be present.

nanging the temperature. 916040 =H₂(g) + Cl₂(g), Kc = 0.290 at 400 K. If 1.50x10³ M of HCL, H₂, and Cl₂ are mixed me of the following will happen? HCl and Cl₂ will increase as the system approaches equilibrium. H₂ and Cl₂ will increase as the system approaches equilibrium. brium. H₂ and HCI will decrease as the system approaches equilibrium. HCI will increase as the system approaches equilibrium. m constant (Kc) for the reaction N₂(g) + 3H₂(g) = 2NH3(g) is 4.34x10³ at 300 °C. ements will be true regarding the system at equilibrium? minate. minate. resent. resent. of products and reactants will be present.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...
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This is just a practice exam. Please explain reasoning for this question. Thank you!
be changed chang the temperature. 2. For the reaction 2HCl(g) = H₂(g) + Cl₂(g), Kc = 0.290 at 400 K. If 1.50x10³ M of HCL, H₂, and Cl₂ are mixed initially at 400 K, which one of the following will happen? a. The concentrations of HCI and Cl₂ will increase as the system approaches equilibrium. The concentrations of H₂ and Cl₂ will increase as the system approaches equilibrium. b. C. The system is at equilibrium. d. The concentrations of H₂ and HCI will decrease as the system approaches equilibrium. e. The concentration of HCI will increase as the system approaches equilibrium. e. 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.
Transcribed Image Text:be changed chang the temperature. 2. For the reaction 2HCl(g) = H₂(g) + Cl₂(g), Kc = 0.290 at 400 K. If 1.50x10³ M of HCL, H₂, and Cl₂ are mixed initially at 400 K, which one of the following will happen? a. The concentrations of HCI and Cl₂ will increase as the system approaches equilibrium. The concentrations of H₂ and Cl₂ will increase as the system approaches equilibrium. b. C. The system is at equilibrium. d. The concentrations of H₂ and HCI will decrease as the system approaches equilibrium. e. The concentration of HCI will increase as the system approaches equilibrium. e. 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.
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The correct option is E, not B. I still don't understand this concept and how to find the right answer. This is a practice quiz and not graded.

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