Consider the following system at equilibrium where delta Ho = -108 kJ, and Kc =

Question

Consider the following system at equilibrium where delta Ho = -108 kJ, and Kc = 77.5, at 600 K: co(g) + CI2(g) rightarrow cocl2(g) If the TEMPERATURE on the equilibrium system is suddenly increased: 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

Since it is an exothermcic reaction, Kc decreases Q is more than K The rxn must run in reverse direction Cl2 conc. will increase..

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