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Consider the following system at equilibrium where H° = -87.9 kJ, and Kc = 83.3 ,...

Consider the following system at equilibrium where 1e502cd7-69d6-45ee-a32d-787ce5febae7.gifH° = -87.9 kJ, and Kc = 83.3 , at 500 K:

PCl3(g) + Cl2(g) 7e50f1f7-d29b-4777-b1ee-365a063b4be8.gifPCl5(g)

If the TEMPERATURE on the equilibrium system is suddenly decreased :

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.
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Answer #1

Answer:-

This question is solved by using the simple concept of Le Chatelier principle which involves shift in the equilibrium on changing the temperature.

The answer is given in the image,

| Answers PQ 3 cg + Uzeg, I PUS4 DH° = -87.9kJ, Kc - 83-3 It is exothermic reaction The value of Kc = A. Increases because sy

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