Reaction $2A + B \to$  product,  rate law is $\frac{{ - d[A]}}{{dt}}\, = \,K[A].$ At a time when $t\, = \,\frac{{{t_{1/2}}}}{{\ln\,2}},$ concentration of the reactant is

In the reaction $2A + B \to {A_2}B$, if the concentration of $A$ is doubled and of $B$ is halved, then the rate of the reaction will

For a chemical reaction,$ A + 2B \to C + D,$ the rate of reaction increases three times, when concentration of $A$ only is increased nine times. While when concentration of $B$ only is increased $2\,times,$ then rate of reaction also increases $2\,times$. The order of this reaction is

If the surface area of the reactants increases, then order of the reaction

$2 NO ( g )+ Cl _{2}( g ) \rightleftharpoons 2 NOCl ( s )$

This reaction was studied at $-10^{\circ} C$ and the following data was obtained

$[ NO ]_{0}$ and $\left[ Cl _{2}\right]_{0}$ are the initial concentrations and $r _{0}$ is the initial reaction rate.

The overall order of the reaction is ..........

(Round off to the Nearest Integer).

In a reaction $2A + B \to {A_2}B$, the reactant $ A $ will disappear at