In a reaction $2A + B \to A_2B$,the reactant $A$ will disappear at

In a reaction $R \to P$,the concentration $[M]$ obtained at different times $(t)$ are shown in the following table. Calculate the average rate $r_{av}$ of the reaction.

Time $t$ $(s)$	$0$	$5$	$10$	$20$	$30$
Concentration $(mol \ L^{-1})$	$160 \times 10^{-3}$	$80 \times 10^{-3}$	$40 \times 10^{-3}$	$10 \times 10^{-3}$	$3.5 \times 10^{-3}$

For the reaction $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$,the rate of formation of $NO_2$ is $\frac{d[NO_2]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of disappearance of $O_2$,i.e.,$-\frac{d[O_2]}{dt}$.

Consider the reaction,$2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$. In the figure below,identify the curves $X, Y$ and $Z$ associated with the three species in the reaction.

Explain how the rate of reaction depends on concentration and time using graphs.

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: