For the reaction,$CH_3Br_{(aq)} + OH_{(aq)}^{-} \longrightarrow CH_3OH_{(aq)} + Br_{(aq)}^{-}$,the rate of consumption of $OH_{(aq)}^{-}$ is $x \ mol \ dm^{-3} \ s^{-1}$. What is the rate of formation of $Br_{(aq)}^{-}$ (in $mol \ dm^{-3} \ s^{-1}$)?

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.,$-\frac{d[O_2]}{dt}$.

For the reaction,$3 I_{(aq)}^{-} + S_2 O_{8_{(aq)}}^{2-} \longrightarrow I_{3_{(aq)}}^{-} + 2 SO_{4_{(aq)}}^{2-}$,the rate of formation of $SO_4^{2-}$ is $0.022 \ mol \ dm^{-3} \ sec^{-1}$. What is the rate of formation of $I_{3_{(aq)}}^{-}$?

For the reaction,$XA + YB \rightarrow ZC$,if $\frac{- d [ A ]}{ dt } = \frac{- d [ B ]}{ dt } = \frac{d [ C ]}{ dt },$ then the correct statement among the following is:

For a chemical reaction $4 A + 3 B \rightarrow 6 C + 9 D$,the rate of formation of $C$ is $6 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$ and the rate of disappearance of $A$ is $4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. The rate of reaction and the amount of $B$ consumed in an interval of $10 \ s$,respectively,will be:

For the reaction $2A + B \rightarrow 3C + D$,which of the following does not express the rate of reaction?