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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For the reaction $N_{2}O_{5(g)} \rightarrow 2NO_{2(g)} + \frac{1}{2} O_{2(g)}$,the rate of disappearance of $N_{2}O_{5}$ is given as $6.25 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of $NO_{2}$ and $O_{2}$ is given respectively as:
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In a reaction,$n_1A + n_2B \to m_1C + m_2D$,$5 \ M$ of reactant $A$ are allowed to react with $3 \ M$ of reactant $B$. After $5 \ sec$,the concentration of $A$ was found to be $4 \ M$. What are the rate of decomposition of $A$ and the rate of formation of $D$,respectively?
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