Consider the reaction n2(g) + o2(g) â 2 no(g) k = 0.0025 a rigid container initially contains 8.00 atm of nitrogen and 5.00 atm of oxygen. what will be the partial pressure of nitrogen at equilibrium?

7.8458 atm

Explanation:

For the reaction  

Kp is defined as:

The conditions in the system are:

                   O2      N2             NO

initial            5 atm     8 atm           0

equilibrium     5-x           8-x              2x

From the stoichiometric relationship in the reaction we know that to produce 2x of NO we need x of N2 and O2.

Replacing the values in the expression for Kp we get

working with this expression

This a quadratic equation with

a=(4-Kp)

b=13*Kp

C=-40*Kp

Replacing the given value for Kp we get:

a=3.9975

b=0.0325

C=-0.1

the solution for this equation is given by the next equation:

we will get to values for X

Since negative partial pressures don't have physical meaning the solution for the system is x=0.1541.

So the partial pressure of nitrogen at the equilibrium is