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Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K.N2(g) + 3H2(g) 2NH3(g)If the TEMPERATURE on the equilibrium system is suddenly increased:The value of Kc A. increases.  B. decreases.  C. remains the same. The value of Q A. is greater than Kc.  B. is equal to Kc.  C. is less than Kc. The reaction must: A. run in the forward direction to reestablish equilibrium.  B. run in the reverse direction to reestablish equilibrium.  C. remain the same. It is already at equilibrium. The concentration of H2 will: A. increase.  B. decrease.  C. remain the same.

Question

Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K.

N2(g) + 3H2(g) 2NH3(g)

If the TEMPERATURE on the equilibrium system is suddenly increased:

The value of Kc   A. increases.
    B. decreases.
    C. remains the same.

 

The value of Q   A. is greater than Kc.
    B. is equal to Kc.
    C. is less than Kc.

 

The reaction must:   A. run in the forward direction to reestablish equilibrium.
    B. run in the reverse direction to reestablish equilibrium.
    C. remain the same. It is already at equilibrium.

 

The concentration of H2 will:   A. increase.
    B. decrease.
    C. remain the same.
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Step 1

The given reaction is...

2NH3(g)
N (g)+3H, (g)
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2NH3(g) N (g)+3H, (g)

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