Thermal decomposition of N_2O_5 occurs as per | vedclass

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(D) For the reaction $2N_2O_5 \longrightarrow 4NO_2 + O_2$,the rate expression is given by:$Rate = -\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \fr

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Rate of disappearance of $N_2O_5$ is twice the $O_2$ production rate

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(D) For the reaction $2N_2O_5 \longrightarrow 4NO_2 + O_2$,the rate expression is given by:$Rate = -\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$From this,we can relate the rate of disappearance of $N_2O_5$ to the rate of production of $O_2$:$-\frac{d[N_2O_5]}{dt} = 2 	imes \frac{d[O_2]}{dt}$Thus,the rate of disappearance of $N_2O_5$ is twice the rate of production of $O_2$.

Thermal decomposition of $N_2O_5$ occurs as per the equation below:
$2N_2O_5 \longrightarrow 4NO_2 + O_2$
The correct statement is:

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Thermal decomposition of $N_2O_5$ occurs as per the equation below:$2N_2O_5 \longrightarrow 4NO_2 + O_2$The correct statement is: