In the following reaction $3A \to B + 2C$,the initial concentration of $A$ is $8\,mol\,L^{-1}$. After $10\,min$,it becomes $5\,mol\,L^{-1}$. Find the rate of reaction in $mol\,L^{-1}\,min^{-1}$.

Write the rate equation for the following reactions:
$1.$ $5 Br^{-}_{(aq)} + BrO^{-}_{3_{(aq)}} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2_{(aq)}} + 3 H_2O_{(l)}$
$2.$ $R \rightarrow P$
$3.$ $C_4H_9Cl + H_2O \rightarrow C_4H_9OH + HCl$

The concentration of a reactant changes from $0.1 \, mol \, L^{-1}$ to $0.095 \, mol \, L^{-1}$ in $10 \, s$. Calculate the rate of reaction.

For a reaction,$2A + B \rightarrow 2C$,the rate of disappearance of $A$ is $0.076 \ mol \ dm^{-3} \ s^{-1}$. What is the rate of disappearance of $B$?

In the hydrogenation of ethene at $298 \, K$,the number of moles of hydrogen decreases from $2.2$ to $1.4$ in $50 \, min$. Calculate the rate of reaction in units of $mol \, s^{-1}$.

In the following reaction: $xA \to yB$,$\log \left[ -\frac{d[A]}{dt} \right] = \log \left[ \frac{d[B]}{dt} \right] + \log 2$,where the negative sign indicates the rate of disappearance of the reactant. Thus,$x : y$ is: