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

Given above is the concentration vs time plot for a dissociation reaction: $A \rightarrow nB$. Based on the data of the initial phase of the reaction (initial $10 \ min$), the value of $n$ is . . . . . . .

Identify the correct expression for the rate of the following reaction: $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$

The reaction given below $2 NH_{3(g)} \xrightarrow{Pt} N_{2(g)} + 3 H_{2(g)}$ has a rate of reaction of $2.5 \times 10^{-6} \ mol \ dm^{-3} \ sec^{-1}$. What is the rate of formation of $H_{2(g)}$?

Consider the following reactant samples:
$I$. $1 \ mol$ of $A$ and $2 \ mol$ of $B$ in a $1 \ L$ vessel
$II$. $2 \ mol$ of $A$ and $2 \ mol$ of $B$ in a $2 \ L$ vessel
$III$. $0.2 \ mol$ of $A$ and $0.2 \ mol$ of $B$ in a $0.1 \ L$ vessel
Which reactant sample reacts at the highest rate if the reactants are in the gaseous state and do not follow a zero-order reaction?

For the reaction ${N_2}_{(g)} + 3{H_2}_{(g)} \to 2N{H_3}_{(g)}$,what is the relationship between $\frac{d[N{H_3}]}{dt}$ and $-\frac{d[{H_2}]}{dt}$?