Okay, so you're assuming it was a chemical explosion and that there was no deformation of the chamber. What if the "explosion" was the sudden expansion of gases superheated by an intense pulse of laser light? What if that superheating converts some nitrogen and oxygen into nitrogen oxides?
n O2 + m N2 --> x NO + y NO2 + z N2O + ...
So, in the case of an "explosion" in an oxygen/nitrogen atmosphere created without an explosive chemical, n can only *decrease*. So, you're going to assume that there had to be a chemical explosive in the chamber and that the chamber held without any deformation? If you're going that far, why do you even bother throwing the ideal gas law into it? You're already throwing out the problem definition for a fancifully creative alternative, why limit yourself to ideal gas laws?
Frankly, your entertainingly conceived problem about a chemical explosive being set off inside a recompression chamber would be fun to solve. Would you like to actually write it up?
(A sample of 10 grams of trinitrotoluene is detonated in an otherwise empty chamber. Before detonation, the remaining volume of the chamber contained a gas mixture of 21.000% O2 and 79.000% N2, and the internal gauge pressure is 10.1325 kPa. The ambient pressure is 101.325 kPa. The chamber is made up of a cylindrical body and hemispherical ends, both with a diameter of 1.5000 meters. The cylindrical portion of the chamber is 2.5000 meters long...)
Let me know when it's done. Be sure to specify the reaction products, otherwise I'll just have to say it's unsolvable and completely miss the point. (Meanwhile, if anyone has any more of these simple problems, we'll do those.)