Which one of the following equations is correct for the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$?

Mention the factors that affect the rate of a chemical reaction.

For the reaction $N_{2}O_{5(g)} \rightarrow 2NO_{2(g)} + \frac{1}{2} O_{2(g)}$,the rate of disappearance of $N_{2}O_{5}$ is given as $6.25 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of $NO_{2}$ and $O_{2}$ is given respectively as:

For the reaction,$2 \ SO_{2} + O_{2} \rightleftharpoons 2 \ SO_{3}$,the rate of disappearance of $O_{2}$ is $2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of appearance of $SO_{3}$ is

In the reaction,$BrO_{3(aq)}^{-} + 5Br_{(aq)}^{-} + 6H^{+} \to 3Br_{2(l)} + 3H_2O_{(l)}$. The rate of appearance of bromine $(Br_2)$ is related to the rate of disappearance of bromide ions as:

The decomposition of $N_{2}O_{5}$ in $CCl_{4}$ at $318 \ K$ has been studied by monitoring the concentration of $N_{2}O_{5}$ in the solution. Initially the concentration of $N_{2}O_{5}$ is $2.33 \ mol \ L^{-1}$ and after $184 \ minutes$,it is reduced to $2.08 \ mol \ L^{-1}$. The reaction takes place according to the equation:
$2N_{2}O_{5(g)} \rightarrow 4NO_{2(g)} + O_{2(g)}$
Calculate the average rate of this reaction in terms of hours,minutes,and seconds. What is the rate of production of $NO_{2}$ during this period?