In a reaction $A_2B_{3(g)} \to A_{2(g)} + \frac{3}{2}B_{2(g)}$,the pressure increases from $60 \ torr$ to $75 \ torr$ in $2.5 \ min$. The rate of disappearance of $A_2B_3$ is ........ $torr \cdot min^{-1}$.

The rate of a gaseous reaction is given by $r = K[x][y]$. If the volume of the reaction vessel is suddenly reduced to $1/4$ of its initial volume,the rate of the reaction will ............

For the reaction $3A \to 2B$,the rate of reaction is expressed as $\frac{+d[B]}{dt} = \dots$

For the reaction $3 A + 2 B \rightarrow C$,which statement is correct $:-$

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

Nitric oxide reacts with $H_2$ according to the reaction: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_2 O_{(g)}$. Identify the correct relation for the rate of disappearance of reactants and the rate of appearance of products.