Nitrogen and oxygen do not react appreciably at room temperature, as illustrated by our atmosphere. but at high temperatures, the reaction below can proceed to a measurable extent. n2(g) + o2(g) ⇔ 2 no(g) at 3000 k, the reaction above has keq = 0.0153. if 0.3152 mol of pure no is injected into an evacuated 2.0-l container and heated to 3000k, what will be the equilibrium concentration of no?

Answer : The equilibrium concentration of NO is, 0.0092 M.

Solution :

First we have to calculate the concentration of NO.

The given equilibrium reaction is,

Initially conc.      0        0           0.1576

At eqm.               (x)       (x)        (0.1576-2x)

The expression of will be,

By solving the term, we get:

Neglecting the 0.0839 value of x because it can not be more than initial value.

Thus, the value of 'x' will be, 0.0742 M

Now we have to calculate the equilibrium concentration of NO.

Equilibrium concentration of NO = (0.1576-2x) = [0.1576-2(0.0742)] = 0.0092 M

Therefore, the equilibrium concentration of NO is, 0.0092 M.