If the instantaneous rate of reaction is stated as $-\frac{1}{2} \frac{d[x]}{dt} = -\frac{d[y]}{dt} = \frac{1}{2} \frac{d[z]}{dt}$,identify the reaction.

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:

From the concentrations of $C_{4}H_{9}Cl$ (butyl chloride) at different times given below,calculate the average rate of the reaction:
$C_{4}H_{9}Cl + H_{2}O \rightarrow C_{4}H_{9}OH + HCl$
during different intervals of time.

$t/s$	$0$	$50$	$100$	$150$	$200$	$300$	$400$	$700$	$800$
$[C_{4}H_{9}Cl]/mol\ L^{-1}$	$0.100$	$0.0905$	$0.0820$	$0.0741$	$0.0671$	$0.0549$	$0.0439$	$0.0210$	$0.017$

In a pseudo first order reaction in water,the following results were obtained:

$t / s$	$0$	$30$	$60$	$90$
$[A] / mol \ L^{-1}$	$0.55$	$0.31$	$0.17$	$0.085$

Calculate the average rate of reaction between the time interval $30$ to $60 \ s$.

For a reaction $\frac{1}{2} A \rightarrow 2 B$,the rate of disappearance of $A$ is related to the rate of appearance of $B$ by the expression:

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?