The equilibrium constant for the reaction
COCl2 (g) CO (g) + Cl2 (g) is Kc = 4.63 ´ 10–3 at 527 °C
If 10 g of COCl2(g) is placed in a 1 L container, determine how much Cl2 is present at equilibrium.

The concentrations of at equilibrium is 0.023 M

Explanation:

Moles of   =

Volume of solution = 1 L

Initial concentration of =

The given balanced equilibrium reaction is,

Initial conc.           0.14 M           0 M       0M    

At eqm. conc.     (0.14-x) M        (x) M        (x) M

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

By solving the term 'x', we get :

x = 0.023 M

Thus, the concentrations of at equilibrium is 0.023 M

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

the answers would be

the first one and the second one