Consider the following system at equilibrium where H° = -16.1 kJ/mol, and Kc = 154 , at 298 K. 2 NO (g) + Br2 (g) 2 NO

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Consider the following system at equilibrium
where H°
= -16.1 kJ/mol, and
Kc = 154 ,
at 298 K.

2 NO (g)
+ Br2 (g) 2 NOBr (g)

When 0.16 moles
of NOBr (g) are added
to the equilibrium system at constant
temperature:

The value of Kc ???? (Increases, decreases, remains
the same)
The value of Qc ???? (is greater than, is equal to,
is less than) Kc.

The reaction must
A. run in the forward direction to restablish equilibrium.
B. run in the reverse direction to restablish equilibrium.
C. remain the same. It is already at equilibrium.
The concentration
of Br2 will ???( increase,
decrease, remain the same.)