At a definite temperature and pressure,the rate of a reaction depends on which of the following factors?

For the elementary reaction $2 SO_{2(g)} + O_{2(g)} \rightarrow 2 SO_{3(g)}$,identify the correct relation among the following.

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 . . . . . . .

At $298 \ K$ the value of $-\frac{\Delta[Br^{-}]}{\Delta t}$ for the reaction$5Br^-{_{\text{(aq)}}} + BrO_3^-{_{\text{(aq)}}} + 6H^+{_{\text{(aq)}}} \rightarrow 3Br_{2\text{(aq)}} + 3H_2O_{\text{(l)}}$ is $x \ mol \ L^{-1} \ min^{-1}$. What is the rate (in $mol \ L^{-1} \ min^{-1}$) of this reaction?

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the reaction occurs under specific temperature and partial pressure conditions. The rate of formation of $NH_3$ is $0.001 \, kg \, h^{-1}$. The rate of consumption of $H_2$ under the same conditions is ...... $kg \, h^{-1}$.

Explain the relation between the rate of reaction and the stoichiometric coefficients of a balanced chemical equation with examples.