If $3A \to 2B$,then the rate of reaction of $+\frac{d[B]}{dt}$ is equal to

Write the rate equation for the following reactions:
$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$

For the reaction: $A + 2 B \rightarrow C + D$,the expression for the rate of reaction is:

The concentration of a reactant decreases from $0.2 \ M$ to $0.1 \ M$ in $10 \ \text{minutes}$. The rate of the reaction is

Consider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) is:

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 $(mol \ L^{-1})$	$160 \times 10^{-3}$	$80 \times 10^{-3}$	$40 \times 10^{-3}$	$10 \times 10^{-3}$	$3.5 \times 10^{-3}$