If the rate of disappearance of N_2O_5 in the | vedclass

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(C) For the reaction $2 \ N_2O_{5(g)} \longrightarrow 4 \ NO_{2(g)} + O_{2(g)}$,the rate expression is given by: $-\frac{1}{2} \frac{d[N_2O_5]}{dt} =

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$2.4 	imes 10^{-5}$

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(C) For the reaction $2 \ N_2O_{5(g)} \longrightarrow 4 \ NO_{2(g)} + O_{2(g)}$,the rate expression is given by: $-\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$ Given that the rate of disappearance of $N_2O_5$ is $-\frac{d[N_2O_5]}{dt} = 1.2 	imes 10^{-5} \ mol \ L^{-1} \ s^{-1}$. From the rate expression,we have: $\frac{d[NO_2]}{dt} = 2 	imes \left(-\frac{d[N_2O_5]}{dt}ight)$ $\frac{d[NO_2]}{dt} = 2 	imes (1.2 	imes 10^{-5}) = 2.4 	imes 10^{-5} \ mol \ L^{-1} \ s^{-1}$.

If the rate of disappearance of $N_2O_5$ in the following reaction is $1.2 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$,the rate of production of $NO_2$ in $mol \ L^{-1} \ s^{-1}$ is:
$2 \ N_2O_{5(g)} \longrightarrow 4 \ NO_{2(g)} + O_{2(g)}$

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If the rate of disappearance of $N_2O_5$ in the following reaction is $1.2 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$,the rate of production of $NO_2$ in $mol \ L^{-1} \ s^{-1}$ is: $2 \ N_2O_{5(g)} \longrightarrow 4 \ NO_{2(g)} + O_{2(g)}$