Consider the following system at equilibrium where AH°=-108 kJ, and K, 77.5, at 600 K. CO(g) + C,(g) COC1,(g) When 0.22 moles of Cl,(g) are added to the equilibrium system at constant temperature: The value of K The value of Q. |K. The reaction must O run in the forward direction to restablish cquilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of CO will
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Consider the following system at equilibrium where AH=-108 kJ, and K. 77.5, at 600 K.
CO(g) + C,(g) COCI,(g)
When 0.22 moles of Cl,(g) are added to the equilibrium system at constant temperature:
The value of K
The value of Qe
K.
The reaction must
O run in the forward direction to restablish cquilibrium.
O run in the reverse direction to restablish cquilibrium.
O remain the same. It is already at cquilibrium.
The concentration of CO will
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The equilibrium constant of the reaction (Kc) = 77.5
Temperature of the reaction (T) = 600K
The given reaction is:
The equilibrium constant Kc is given by:
If 0.22 moles of Cl2(g) is added to the system in equilibrium :
Cl2(g) is present on reactants side. Reactants are present in denominator. So by increasing the concentration of reactant results in decreasing the value of equilibrium constant (Kc).
But at a given temperature the equilibrium constant of a reaction remains constant. So in order maintain Kc value as 77.5 the concentration of product (COCl2(g)) increases to nullify the change.
This results in increase in concentration of products and the equilibrium shift the reaction towards forward direction.
Therefore, at constant temperature the equilibrium of a reaction remains constant.
The value of Kc remains constant.
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