If the rate of disappearance of N_2O_5 in the | vedclass

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

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$2.4 	imes 10^{-5}$

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(C) For the reaction $2N_2O_{5(g)} \longrightarrow 4NO_{2(g)} + O_{2(g)}$,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{1}{4} \frac{d[NO_2]}{dt} = \frac{1}{2} \left( -\frac{d[N_2O_5]}{dt} ight)$$\frac{d[NO_2]}{dt} = 2 	imes \left( -\frac{d[N_2O_5]}{dt} ight)$$\frac{d[NO_2]}{dt} = 2 	imes (1.2 	imes 10^{-5} \ mol \ L^{-1} \ s^{-1}) = 2.4 	imes 10^{-5} \ mol \ L^{-1} \ s^{-1}$.

$t / s$	$0$	$30$	$60$	$90$
$[A] / mol \ L^{-1}$	$0.55$	$0.31$	$0.17$	$0.085$

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:
$2N_2O_{5(g)} \longrightarrow 4NO_{2(g)} + O_{2(g)}$

Similar Questions

For the reaction,$A + 3 B \rightarrow 2 C$,the rate of consumption of $A$ is $1.4 \ mol \ dm^{-3} \ minute^{-1}$. Calculate the rate of consumption of $B$.

The rate of reaction is expressed as
$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$
The reaction is:

In the reaction $2 N_{2}O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the ratio of the rate of formation of $NO_{2(g)}$ to the rate of formation of $O_{2(g)}$ is:

In a pseudo first order reaction in water,the following results were obtained:

$t / s$ $0$ $30$ $60$ $90$

$[A] / mol \ L^{-1}$ $0.55$ $0.31$ $0.17$ $0.085$

Calculate the average rate of reaction between the time interval $30$ to $60 \ s$.

For the reaction $CH_3COOCH_3 + H_2O \xrightarrow{H^{+}} CH_3COOH + CH_3OH$,the progress of the reaction is followed by:

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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:$2N_2O_{5(g)} \longrightarrow 4NO_{2(g)} + O_{2(g)}$