For the reaction $3 \,A \rightarrow 2 \,B$, the rate of reaction $+\frac{d[B]}{d t}$ is equal to:

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

Observe the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?

Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

For the reaction,$2 \ NO_{(g)} + O_{2_{(g)}} \rightarrow 2 \ NO_{2_{(g)}}$. If $\frac{d[NO_2]}{dt} = 0.052 \ mol \ dm^{-3} \ s^{-1}$,calculate the rate of consumption of $NO_{(g)}$.

For the reaction $2 \ NO + Cl_2 \rightarrow 2 \ NOCl$,what is the relation between $\frac{d[NO]}{dt}$ and $\frac{d[NOCl]}{dt}$?