The rate of a gaseous reaction is given by the expression $K [A] [B]$. If the volume of the reaction vessel is suddenly reduced to $1/4$ of the initial volume,the reaction rate relating to the original rate will be

For a reaction,$A + B \rightarrow \text{Product}$; the rate law is given by,$r = k[A]^{1/2}[B]^2$. What is the order of the reaction?

If in a certain reaction,two different reactants take part,then:

The initial reaction $2AB + B \to A_2B_3$ is carried out in vessels of volume $1 \ dm^3$ and $2 \ dm^3$ respectively,using equal moles of reactants. The ratio of the reaction rates $(r_1/r_2)$ is:

In the hydrolysis of an organic chloride in the presence of a large excess of water,the reaction is $RCl + H_2O \longrightarrow ROH + HCl$. Determine the molecularity and order of the reaction.

$A$ reaction $2A + B \xrightarrow{k} C + D$ is first order with respect to $A$ and second order with respect to $B$. Initial concentration $(t = 0)$ of $A$ is $C_0$ while $B$ is $2C_0$. If at $t = 30 \min$ the concentration of $C$ is $C_0/4$,then the rate expression at $t = 30 \min$ is: