5 14 points 0 My Notes Ask Your Teacher Nitrogen dioxide dec

5. -14 points 0 My Notes Ask Your Teacher Nitrogen dioxide decomposes according to the reaction given below where Kp 4.48 x 10-13 at a certain temperature. 2 NO2(9)2 NO(g)+O2(9) A pressure of 0.89 atm of NO2 is introduced into a container and allowed to come to equilibrium. What are the equilibrium partial pressures of NO(g) and O2(9)? PNo 40 Po2 atm atm

Solution

2 NO2   <-------------> 2 NO (g) + O2 (g)

0.89 atm                       0                   0

0.89 - 2x                       2x                  x

Kp = (2x)^2(x) / (0.89 - 2x)^2

4.48 x 10^-13 = 4x^3 / (0.89 - 2x)^2

x = 4.46 x 10^-5

At equilibrium :

P_NO = 8.9 x 10^-5 atm

P_O2 = 4.5 x 10^-5 atm