Consider the following system a equilibrium where delta H degree = 108 kJ, and K

Question

Consider the following system a equilibrium where delta H degree = 108 kJ, and K_c = 77.5. at 600 K. CO(g) + Cl-@(g) COCL_2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of K_c A. increases B. decreases. C. remains the same The value of Q_c A. is greater than K_c. B. is equal to K_c. C. is less than K_c. The reaction must A run in the forward direction to reestablish equilibrium B. run in the reverse direction to reestablish equilibrium C. remain the same. It is already at equilibrium The number of moles of Cl_2 will A increase B. decrease C remain the same

Explanation / Answer

The valur of Kc will definitely increase as it is defined as the ratio of concentration of products to that of reactants, and by increasing the volume of system the decrease in reactant concentration is more compared to that of product.

Value of Qc will be greater than Kc

The reaction will move in the reverse direction and the no. Of moles of Cl2 will increase according to the Le Chatelier's principle.

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