Consider the following system at equilibrium where H = -108 kJ, and Kc= 77.5, at

Question

Consider the following system at equilibrium where H = -108 kJ, and Kc= 77.5, at 600 K: CO(g) + Cl2(g) COCI2(g) When 0.27 moles of COCI2(g) are added to the equilibrium system at constant temperature: The value of Kc Increases Decreases Remains the same The value of Q Is greater than K Is equal to K Is less than K The reaction must: Run in the forward direction to restablish equilibrium. Run in the reverse direction to restablish equilibrium. Remain the same. Already at equilibrium. The concentration of Cl2 will: Increase. Decrease. Remain the same.

Explanation / Answer

C, A, B, A

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---