At 100°C, Kp = 60.6 for the reaction 2 NOBr(g) ⇌ 2 NO(g) + Br2(g) In a given experiment, 1.75 atm of each component is placed in a container. Is the system at equilibrium? If not, in which direction will the reaction proceed?

The system is not at equilibrium.

The reaction will proceed to the right to attain the equilibrium.

Explanation:

Let's consider the following reaction.

2 NOBr(g) ⇌ 2 NO(g) + Br₂(g)

The pressure equilibrium constant (Kp) is 60.6. To determine if the system is at equilibrium when the pressure of each component is 1.75 atm, we have to calculate the reaction quotient (Q) and compare it with Kp.

Q = [NO]².[Br₂] / [NOBr]²

Q = (1.75)².(1.75) / (1.75)²

Q = 1.75

Since Q ≠ Kp, the system is not at equilibrium.

Since Q < Kp, the reaction will proceed to the right to attain the equilibrium.

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