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 22 seconds and 0.54 M-1 s-1, respectively, how many moles of NO2 were in the original sample?

Question

Chemistry

Skylar Reese

11 December, 21:37

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 22 seconds and 0.54 M-1 s-1, respectively, how many moles of NO2 were in the original sample?

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Kara Kirby · Answer 1

T (1/2) = 1 / (k[NO2])

[NO2]=1 / (kt (1/2))

[NO2]=1 / (0.54M-1 s-1*22s) seconds cancel

[NO2]=1/11.88=0.0842

inital mole = 0.0842*volume (2.5) = 0.210 mols