For the reaction $2 N_2O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$,the initial concentration of $N_2O_5$ is $2.0 \ mol \ L^{-1}$ and after $300 \ min$,it is reduced to $1.4 \ mol \ L^{-1}$. The rate of production of $NO_2$ (in $mol \ L^{-1} \ min^{-1}$) is

For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the rate of reaction is expressed as:

Ammonia and oxygen react at high temperature as in the reaction,$4 NH_{3(g)} + 5 O_{2(g)} \rightarrow 4 NO_{(g)} + 6 H_2O_{(g)}$. If the rate of formation of $NO$ is $3.6 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1}$,calculate the rate of formation of water.

In the reaction,$N_{2} + 3H_{2} \longrightarrow 2NH_{3}$,the rate of disappearance of $H_{2}$ is $0.02 \ M/s$. The rate of appearance of $NH_{3}$ is (in $M/s$)

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?

For a chemical reaction $A \rightarrow B$,it was found that the concentration of $B$ increases by $0.2 \, mol \, L^{-1}$ in $30 \, min$. The average rate of the reaction is $...... \times 10^{-1} \, mol \, L^{-1} \, h^{-1}$. (Nearest integer)