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

Consider the reaction, $3I^-_{(aq)} + S_2O_8^{2-} (aq) \rightarrow I_3^- (aq) + 2SO_4^{2-} (aq)$. If the rate of formation of $SO_4^{2-}$ at a particular time is $2.2 \times 10^{-2} \text{ mol dm}^{-3} \text{s}^{-1}$, calculate the rate of consumption of $I^-$.

The instantaneous rate of a reaction is given by $-\frac{1}{2} \frac{d[x]}{dt} = -\frac{d[y]}{dt} = \frac{1}{2} \frac{d[z]}{dt}$. Identify the reaction.

In a reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of appearance of $NH_3$ is $2.5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$. The rate of reaction and rate of disappearance of $H_2$ will be (in $mol \ L^{-1} s^{-1}$):

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.

For the reaction $5Br_{(aq)}^{-} + BrO_{3_{(aq)}}^{-} + 6H_{(aq)}^{+} \rightarrow 3Br_{2_{(aq)}} + 3H_{2}O_{(l)}$,if $\frac{-\Delta[Br^{-}]}{\Delta t} = 4.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,calculate the rate of formation of $Br_{2}$,i.e.,$\frac{\Delta[Br_{2}]}{\Delta t}$.