The following results were obtained during kinetic studies of the reaction $2A+B$ $\to$ products

Experiment	$[A]$ (in $mol\, L^{-1})$	$[B]$ (in $mol\, L^{-1})$	Initial rate of reaction (in $mol\, L^{-1}\,min^{-1})$
$I$	$0.10$	$0.20$	$6.93 \times {10^{ - 3}}$
$II$	$0.10$	$0.25$	$6.93 \times {10^{ - 3}}$
$III$	$0.20$	$0.30$	$1.386 \times {10^{ - 2}}$

The time(in minutes) required to consume half of $A$ is

The hydrolysis of ethyl acetate is a reaction of ......... order

$C{{H}_{3}}COOEt+{{H}_{2}}O\xrightarrow{{{H}^{+}}}C{{H}_{3}}COOH+EtOH$

In a chemical reaction $A$ is converted into $B$ . The rates of reaction, starting with initial concentrations of $A$ as $2 \times {10^{ - 3}}\,M$ and $1 \times {10^{ - 3}}\,M$ , are equal to $2.40 \times {10^{ - 4}}\,M{s^{ - 1}}$ and $0.60 \times {10^{ - 4}}\,M{s^{ - 1}}$ respectively. The order of reaction with respect to reactant $A$ will be

For a reaction of order $\mathrm{n}$, the unit of the rate constant is :

For a particular reaction, the rate expression is given as $r = k[A] [B]^{0.5}$. If the volume of vessel is reduced to one-fourth of the initial volume, the rate of reaction would

For a reaction $\mathrm{A} \xrightarrow{\mathrm{K}_4} \mathrm{~B} \xrightarrow{\mathrm{K}_2} \mathrm{C}$

If the rate of formation of $B$ is set to be zero then the concentration of $B$ is given by :