For the reaction,$2 N_2O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$,$N_2O_5$ disappears at a rate of $x \ mol \ dm^{-3} \ s^{-1}$. Find the rate of formation of $O_2$?
- A$x \ mol \ dm^{-3} \ s^{-1}$
- B$2x \ mol \ dm^{-3} \ s^{-1}$
- C$\frac{x}{2} \ mol \ dm^{-3} \ s^{-1}$
- D$\frac{3x}{2} \ mol \ dm^{-3} \ s^{-1}$
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