At a certain temperature, 4.0 mol NH3 is introduced into a 2.0 L container, and the NH3 partially dissociates by the reaction below. 2 NH3(g) equilibrium reaction arrow N2(g) 3 H2(g) At equilibrium, 2.0 mol NH3 remains. What is the value of K for this reaction

The value of K for this reaction is 1.6875

Explanation:

Moles of   = 4.0 mole

Volume of solution = 2.0 L

Initial concentration of =

The given balanced equilibrium reaction is,

Initial conc.          2 M           0 M         0 M

At eqm. conc.     (2-2x) M   (x) M   (3x) M

Equilibrium concentration of =

The expression for equilibrium constant for this reaction will be,

(2-2x) = 1.0

x= 0.5 M

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

Thus the value of K for this reaction is 1.6875