consider the following system at equilibrium where h 108 kj and kc 12910 2 at 600 k cocl2g cog c

First, let's consider the first system. The reaction is exothermic (ΔH° = 108 kJ/mol), meaning i

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Consider the following system at equilibrium where ΔH° = 108 kJ/mol and Kc = 1.29×10^-2 at 600 K. COCl2(g) ⇌ CO(g) + Cl2(g) When 0.20 moles of CO(g) are removed from the equilibrium system at constant temperature, the value of Kc remains the same. The reaction must run in the reverse direction to reestablish equilibrium. The concentration of Cl2 will decrease. Consider the following system at equilibrium where ΔH° = -108 kJ/mol and Kc = 77.5 at 600 K. CO(g) + Cl2(g) ⇌ COCl2(g) When 0.33 moles of COCl2(g) are removed from the equilibrium system at constant temperature, the value of Kc remains the same. The value of Qc is less than Kc. The reaction must run in the forward direction to reestablish equilibrium. The concentration of Cl2 will decrease.

          Consider the following system at equilibrium where ΔH° = 108 kJ/mol and Kc = 1.29×10^-2 at 600 K. 
COCl2(g) ⇌ CO(g) + Cl2(g) 
When 0.20 moles of CO(g) are removed from the equilibrium system at constant temperature, the value of Kc remains the same. The reaction must run in the reverse direction to reestablish equilibrium. The concentration of Cl2 will decrease.

Consider the following system at equilibrium where ΔH° = -108 kJ/mol and Kc = 77.5 at 600 K. 
CO(g) + Cl2(g) ⇌ COCl2(g) 
When 0.33 moles of COCl2(g) are removed from the equilibrium system at constant temperature, the value of Kc remains the same. The value of Qc is less than Kc. The reaction must run in the forward direction to reestablish equilibrium. The concentration of Cl2 will decrease.

Added by Carmen P.

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