Consider the following system at equilibrium where ΔΗ° - 111 kJ, and == Kc = 0.159, at 7.23 × 10² K: N₂ (9) + 3H₂ (9) — 2NH3 (g) If the temperature on the equilibrium system is suddenly decreased: The value of Kc Oincreases Odecreases Oremains the same The value of Qc is less than Ke Ois greater than Ko Ois equal to Ke The reaction must run in the forward direction to reestablish equilibrium run in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of H₂ will Oincrease decrease Oremain the same

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Consider the following system at equilibrium where 
\(\Delta H^\circ = -111 \, \text{kJ}\), and 
\(K_c = 0.159\), at 
\(7.23 \times 10^2 \, \text{K}\):

\[ 
\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) 
\]

If the temperature on the equilibrium system is suddenly decreased:

**The value of \(K_c\):**  
- ⬤ increases  
- ○ decreases  
- ○ remains the same  

**The value of \(Q_c\):**  
- ○ is less than \(K_c\)  
- ○ is greater than \(K_c\)  
- ○ is equal to \(K_c\)  

**The reaction must:**  
- ○ run in the forward direction to reestablish equilibrium  
- ○ run in the reverse direction to reestablish equilibrium  
- ○ remain in the current position, since it is already at equilibrium  

**The concentration of \(\text{H}_2\) will:**  
- ○ increase  
- ○ decrease  
- ○ remain the same
Transcribed Image Text:Consider the following system at equilibrium where \(\Delta H^\circ = -111 \, \text{kJ}\), and \(K_c = 0.159\), at \(7.23 \times 10^2 \, \text{K}\): \[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \] If the temperature on the equilibrium system is suddenly decreased: **The value of \(K_c\):** - ⬤ increases - ○ decreases - ○ remains the same **The value of \(Q_c\):** - ○ is less than \(K_c\) - ○ is greater than \(K_c\) - ○ is equal to \(K_c\) **The reaction must:** - ○ run in the forward direction to reestablish equilibrium - ○ run in the reverse direction to reestablish equilibrium - ○ remain in the current position, since it is already at equilibrium **The concentration of \(\text{H}_2\) will:** - ○ increase - ○ decrease - ○ remain the same
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