For the reaction $N_{2(g)} + 3 H_{2(g)} \rightarrow 2 NH_{3(g)}$,what is the relation between $\frac{d[N_2]}{dt}$ and $\frac{d[H_2]}{dt}$?

Which are the units of rate of reaction?

In a catalytic conversion of $N_2$ to $NH_3$ by Haber's process,the rate of reaction was expressed as change in the concentration of ammonia per time is $40 \times 10^{-3} \ mol \ L^{-1} s^{-1}$. If there are no side reactions,the rate of the reaction as expressed in terms of hydrogen is (in $mol \ L^{-1} s^{-1}$)

For the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$,under certain conditions of temperature and partial pressure of the reactants,the rate of formation of $NH_3$ is $0.001 \ kg \ h^{-1}$. The rate of conversion of $H_2$ under the same conditions is:

Consider the following reaction: $2 NO_{2(g)} + F_{2(g)} \longrightarrow 2 NO_2F_{(g)}$. The expression for the rate of reaction in terms of the rate of change of partial pressure of reactant and product is/are:

The following results are obtained in the hydrolysis of chlorobutane $(C_4H_9Cl)$:

Time $(s)$	$0$	$100$	$200$	$300$	$400$	$700$	$800$
$[C_4H_9Cl]$ $(mol \, L^{-1})$	$0.100$	$0.082$	$0.067$	$0.055$	$0.044$	$0.021$	$0.017$

Calculate the average rate $r_{av}$ of the reaction during different time intervals.