Nitrogen dioxide decomposes at 300°C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation.
2 NO2(g) → 2 NO(g) + O2(g).
A sample of NO2(g) is initially placed in a 2.50-L reaction vessel at 300°C. If the half-life and the rate constant at 300°C are 11 seconds and 0.54 M-1 s-1, respectively, how many moles of NO2 were in the original sample?
I just need an idea on how to approach this problem.

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How about the second order rate law equation?

Well, I was talking about this equation\[1 / [A]_{t}^{} = 1/[A]_{0}^{} + kt\]

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