1. The problem statement, all variables and given/known data An atmospheric chemist fills a gas-reaction container with gaseous dinitrogen pentaoxide to a pressure of 130. kPa, and the gas decomposes to nitrogen dioxide and oxygen. What is the partial pressure of nitrogen dioxide, PNO2, (in kPa) when the total pressure is 166 kPa? 2. Relevant equations 2(N2O5) --> 2(N2O2) + 3(O2) rate=k[N2O5] Dalton's law of Partial Pressure 3. The attempt at a solution P1=130Kpa P2=166Kpa PNO2=? Not sure where to start. There is no mention of this in this chapter. I can't use regular gas laws because I am not given any volumes or temperatures.