At high temperatures nitrogen dioxide decomposes into nitrogen oxide and oxygen gas according to \ce{2 NO_2 -> 2 NO + O_2}
I have a question now. Let's say at a certain temperature I'm given data for the formation of \ce{O_2}. For example:
At t = 0 we have [\ce{O_2}] = 0 mol/L, at t = 50, [\ce{O_2}] = 7.10 \cdot 10^{-4} mol/L, at t = 100, [\ce{O_2}] = 1.205 \cdot 10^{-3} and so on until a certain time.
If I'm given that the initial concentration of \ce{NO_2} is 0.006M, how can I know what the concentration of \ce{NO_2} is at certain times? I'm asked to determine the order of the reaction on the basis of the given data, and also to present graphically the rate constant.
To do that I need to know if \ln([\ce{NO_2}]) versus time t is a straight line. But how to find [\ce{NO_2}] in the first place?
