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 $O_2$?

Write the rate equation for the following reactions:
$1.$ $5 Br^{-}_{(aq)} + BrO^{-}_{3_{(aq)}} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2_{(aq)}} + 3 H_2O_{(l)}$
$2.$ $R \rightarrow P$
$3.$ $C_4H_9Cl + H_2O \rightarrow C_4H_9OH + HCl$

For the reaction $R \to P$,describe the nature of the graphs of $[R]$ versus $time$ and $[P]$ versus $time$.

In the hydrogenation of ethene at $298 \, K$,the number of moles of hydrogen decreases from $2.2$ to $1.4$ in $50 \, min$. Calculate the rate of reaction in units of $mol \, s^{-1}$.

For the chemical reaction $A + 2B \to 3C$,which of the following expressions correctly represents the rate of reaction?

$NO_2$ required for a reaction is produced by the decomposition of $N_2O_5$ in $CCl_4$ as per the equation $2N_2O_{5(g)} \to 4NO_{2(g)} + O_{2(g)}$. The initial concentration of $N_2O_5$ is $3.00 \, mol \, L^{-1}$ and it is $2.75 \, mol \, L^{-1}$ after $30 \, minutes$. The rate of formation of $NO_2$ is ............... $mol \, L^{-1} \, min^{-1}$