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Consider the following system at equilibrium where AHⓇ = 2NOBr(g) → 2NO(g) + Br₂ (9) When 0.36 moles of NO(g) are added to the equilibrium system at constant temperature: The value of K O increases O decreases O remains the same The value of Q is greater than Ke is equal to Ke is less than Ke 16.1 kJ, and K = 0.00650, at 298 K: The reaction must O run in the forward direction to reestablish equilibrium O run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of NO will increase decrease remain the same

Consider the following system at equilibrium where AHⓇ = 2NOBr(g) → 2NO(g) + Br₂ (9) When 0.36 moles of NO(g) are added to the equilibrium system at constant temperature: The value of K O increases O decreases O remains the same The value of Q is greater than Ke is equal to Ke is less than Ke 16.1 kJ, and K = 0.00650, at 298 K: The reaction must O run in the forward direction to reestablish equilibrium O run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of NO will increase decrease remain the same

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider the following system at equilibrium where AH° = 16.1 kJ, and K = 0.00650, at 298 K: 2NOBr(g) → 2NO(g) + Br₂ (g) When 0.36 moles of NO(g) are added to the equilibrium system at constant temperature: The value of K O increases decreases remains the same The value of Qc O is greater than K O is equal to Ke O is less than Ke The reaction must Orun in the forward direction to reestablish equilibrium run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of NO will increase decrease O remain the same
Transcribed Image Text:Consider the following system at equilibrium where AH° = 16.1 kJ, and K = 0.00650, at 298 K: 2NOBr(g) → 2NO(g) + Br₂ (g) When 0.36 moles of NO(g) are added to the equilibrium system at constant temperature: The value of K O increases decreases remains the same The value of Qc O is greater than K O is equal to Ke O is less than Ke The reaction must Orun in the forward direction to reestablish equilibrium run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of NO will increase decrease O remain the same
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Reverse reaction leads to decrease in concentration of product molecules. when Qc > Kc then equilibrium shift towards left direction. 

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