For the reaction,$2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$,if $\frac{-d[NO_2]}{dt}$ is $1.3 \times 10^{-5} \ mol \ L^{-1} \ sec^{-1}$,what is the rate of formation of $O_2$?
- A$1.3 \times 10^{-6} \ mol \ L^{-1} \ sec^{-1}$
- B$3.25 \times 10^{-6} \ mol \ L^{-1} \ sec^{-1}$
- C$1.62 \times 10^{-6} \ mol \ L^{-1} \ sec^{-1}$
- D$6.5 \times 10^{-6} \ mol \ L^{-1} \ sec^{-1}$
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MediumKVPY 2010
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