Consider the following system at equilibrium where ?11° 879 kJ, and Kc-833, at 5
ID: 1040661 • Letter: C
Question
Consider the following system at equilibrium where ?11° 879 kJ, and Kc-833, at 500 K: PCl3 (g) +Cl2 (g)PCI5 (g) If the TEMPERATURE on theequibium system is suddenly decreased The value of KcA. Increases B. Decreases C. Remains the same A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The value of Qc 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 C2 will:A. Increase. B. Decrease C. Remain the same.Explanation / Answer
1)
Decreasing Temperature will shift the reaction in a direction which release heat as per Le chatelier Principle
Forward reaction is exothermic in nature
hence, forward reaction will be favoured
So, Equilibrium moves to product side and hence Kc increases
Answer: A
2)
Since. Kc has increased, Qc will become less than Kc
Answer: C
3)
Since Qc is less than Kc, reaction will proceed in forward direction
Answer: A
4)
Since reaction move in forward direction, concentration of reactant will decrease and Cl2 is reactant, its concentration will decrease
Answer: B