It is known that at 475K and a total pressure 1Bar, 5% NO
2 is dissociated by follwing reaction:
2NO
2 2NO + O
2Q: 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:
2NO
2 2NO + O
21 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?