An indicator '$X$' is used for studying the effect of variation in concentration of iodide on the rate of reaction of iodide ion with $H_2O_2$ at room temperature. The indicator '$X$' forms a blue-colored complex with compound '$A$' present in the solution. The indicator '$X$' and compound '$A$' respectively are:

For the chemical reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of reaction can be expressed in terms of the concentration of $N_{2(g)}$,$H_{2(g)}$,or $NH_{3(g)}$ with respect to time. Identify the correct relationship between these rates.

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 the reaction $H_2 + I_2 \rightarrow 2HI$,state the correct differential rate law.

For the reaction $2A + 3B \to 4C$,the rate of reaction may be represented as:

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: