We’re being asked to calculate the equilibrium constant of HA if a 0.0538 M solution is 3.57% ionized.
Recall that the percent ionization is given by:
The dissociation is as follows:
N2O4(g) ⇌ 2NO2(g)
From this, we can construct an ICE table. Remember that liquids are ignored in the ICE table and Ka expression.
The Kc expression for is:
Note that each concentration is raised by the stoichiometric coefficient: [NO2] is raised to 2 and [N2O4] is raised to 1.
Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation
N2O4(g) ⇌ 2NO2(g).
If at equilibrium N2O4 is 28.0% dissociated, what is the value of the equilibrium constant, Kc, for the reaction under these conditions?
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 Bayer's class at UCF.