At 1000 deg. K, a sample of pure NO2 gas decomposes.
2NO2(g)f/r2NO(g) + O2(g)
The equilibrium constant Kp is 158. analysis shows that the partial pressure of O2 is 0.14 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture in atm.
2NO2(g) f/r 2NO(g) + O2(g)
delta(n_gas) = (2+1) - 2 = 1
P(O2) = 0.14 ...
It shows how to calculate the partial pressures of gases after NO2 decomposes. The solution was rated '5/5' by the student who posted the question originally.