For the reaction,$2N_2O_{5(g)} \rightarrow 4NO_{2(g)} + O_{2(g)}$,the rate of formation of $O_2$ is $0.032 \ g \ h^{-1}$. What is the rate of conversion of $N_2O_5$ in $g \ h^{-1}$?

If the instantaneous rate of reaction is given as $-\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$,then the reaction is represented as:

In the reaction $2SO_3 \to 2SO_2 + O_2$,initially $40 \ g$ of $SO_3$ is heated in a $100 \ mL$ container. If after $10 \ min$,$3.2 \ g$ of $O_2$ is formed,find the rate of reaction in $mol \ L^{-1} \ min^{-1}$.

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

For the reaction $2A + 3B \rightarrow 4C$,the rate of reaction is expressed as:

For a given reaction $3A + B \to C + D$,the rate of reaction can be represented by: