🤓 Based on our data, we think this question is relevant for Professor Li & Thompson's class at PURDUE.
We’re given the following equilibrium reaction:
2 NO2(g) ⇌ 2 NO(g) + O2(g); Kp = 4.48×10−13
Construct an ICE table:
The Kp expression for the reaction is:
Nitrogen dioxide decomposes according to the reaction
2 NO2(g) ⇌ 2 NO(g) + O2(g)
where Kp = 4.48×10−13 at a certain temperature. If 0.75 atm of NO2 is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO(g) and O2(g)?