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

For the reaction $CH_3COOCH_3 + H_2O \xrightarrow{H^{+}} CH_3COOH + CH_3OH$,the progress of the reaction is followed by:

For the reaction $6H^+ + BrO_3^- + 5Br^- \to 3Br_2 + 3H_2O$,which of the following relations is correct for the rate of consumption and formation of products?

Consider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) 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 $mol \ L^{-1} \ min^{-1}$)?

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