What is the rate of formation of $O_2$ for the reaction stated below?
$2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$
Given: $\left| \frac{d[N_2O_5]}{dt} \right| = 0.02 \ mol \ dm^{-3} \ s^{-1}$
$2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$
Given: $\left| \frac{d[N_2O_5]}{dt} \right| = 0.02 \ mol \ dm^{-3} \ s^{-1}$
- A$0.01 \ mol \ dm^{-3} \ s^{-1}$
- B$0.02 \ mol \ dm^{-3} \ s^{-1}$
- C$0.03 \ mol \ dm^{-3} \ s^{-1}$
- D$0.04 \ mol \ dm^{-3} \ s^{-1}$
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