Answer : The partial pressure of  at equilibrium is, 1.0 × 10⁻⁶
 at equilibrium is, 1.0 × 10⁻⁶
Explanation :
The partial pressure of  =
 = 
The partial pressure of  =
 = 
The partial pressure of  =
 = 

The balanced equilibrium reaction is,
                                 
Initial pressure     1.0×10⁻²       2.0×10⁻⁴      2.0×10⁻⁴
At eqm.            (1.0×10⁻²-2p)   (2.0×10⁻⁴+p)  (2.0×10⁻⁴+p)
The expression of equilibrium constant  for the reaction will be:
 for the reaction will be:

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


The partial pressure of  at equilibrium = (2.0×10⁻⁴+(-1.99×10⁻⁴) )= 1.0 × 10⁻⁶
 at equilibrium = (2.0×10⁻⁴+(-1.99×10⁻⁴) )= 1.0 × 10⁻⁶
Therefore, the partial pressure of  at equilibrium is, 1.0 × 10⁻⁶
 at equilibrium is, 1.0 × 10⁻⁶