If the first order reaction involves gaseous reactants and gaseous products,the units of its rate are:

$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:

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,$2 N_2O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$,$N_2O_5$ disappears at a rate of $x \ mol \ dm^{-3} \ s^{-1}$. Find the rate of formation of $O_2$?

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?

Consider the reaction $3 I^{-} + S_2 O_8^{2-} \longrightarrow I_3^{-} + 2 SO_4^{2-}$. At a particular time $t$,$\frac{d[SO_4^{2-}]}{dt}$ is $2.2 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$. What is the value of $\frac{d[S_2 O_8^{2-}]}{dt}$?