Question

Consider the following system at equilibrium where H° = -108 kJ, and K_c = 77.5 , at 600 K:

CO (g) + Cl₂(g) COCl₂(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 Qc		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 restablish equilibrium.
		B. Run in the reverse direction to restablish equilibrium.
		C. Remain the same. Already at equilibrium.

The concentration of Cl2 will:		A. Increase.
		B. Decrease.
		C. Remain the same.

Answer 1

Increasing Temperature will shift the reaction in a direction which absorbs heat as per Le chatelier Principle

Forward reaction is exothermic in nature

hence, backward reaction will be favoured

So, Equilibrium moves to reactant side

Kc would decrease

1)

The value of Kc B

Answer: B

2)

Since Kc decreases, Qc must be greater than Kc

Answer: A

3)

Since Qc > Kc, the reaction runs in backward direction.

Answer: B

4)

Reaction runs in reverse direction and Cl2 is reactant.

So, concentration of Cl2 increases.

Answer: A