[linkamfai]

It is known that at 475K and a total pressure 1Bar, 5% NO₂ is dissociated by follwing reaction:

2NO₂  2NO + O₂



Q:  Keeping the teperature and the total pressure constant, some N2 is added to the system and allowed to reach equilibrium. It is measured that the final partial pressure of N2 is 33.775 kPa. Calculate the NO2 degree of dissociation.


So I try to solve it by:

2NO₂            2NO   +   O₂
1                                             0                  0                   For initial pressure
0.95                                         0.05              0.025         total = 1.025

K= [0.05*1bar/1.025]^2 [0.025*1bar/1.025]/[0.15*1bar/1.025]^2
 = 6.756x10^-5


N2 is added to the system.

N2+O2     2NO



Don't what to do in next step, the equilibrium constant of N2 + O2  2NO is not given

Anyone know how to do?

[Borek]

Don't what to do in next step, the equilibrium constant of N2 + O2  2NO is not given

Sure it is:

It is known that at 475K and a total pressure 1Bar, 5% NO₂ is dissociated

[mjc123]

the equilibrium constant of N2 + O2  2NO is not given

N₂ does not react (under ordinary conditions). It is simply an inert diluent.
Given the constant total pressure, and the stated equilibrium pressure of N₂, what is the total pressure of NO₂, NO and O₂?
Work out the expression for the equilibrium constant as you did before, assuming a fractional conversion of x. You will get an equation in x to solve.

[linkamfai]

the equilibrium constant of N2 + O2  2NO is not given

N₂ does not react (under ordinary conditions). It is simply an inert diluent.
Given the constant total pressure, and the stated equilibrium pressure of N₂, what is the total pressure of NO₂, NO and O₂?
Work out the expression for the equilibrium constant as you did before, assuming a fractional conversion of x. You will get an equation in x to solve.

Thank u, it is useful to me!