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)?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Li & Thompson's class at PURDUE.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.