What is the average rate of reaction when the change in concentration of product is $0.05 \ M$ in $20 \ s$ (in $M \ s^{-1}$)?

For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the rate of reaction is expressed as:

The rate of reaction is expressed as
$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$
The reaction is:

In a reaction,$2X \to Y$,the concentration of $X$ decreases from $0.50 \ M$ to $0.38 \ M$ in $10 \ min$. What is the rate of reaction in $M s^{-1}$ during the interval?

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.

For the reaction,$3 I_{(aq)}^{-} + S_2 O_{8_{(aq)}}^{2-} \longrightarrow 2 SO_{4_{(aq)}}^{2-} + I_{3_{(aq)}}^{-}$,the rate of formation of $SO_{4_{(aq)}}^{2-}$ is $0.044 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of consumption of $I_{(aq)}^{-}$.