Determine the order of reaction on the basis of following data for the reaction $A + B \to C$

Exp.	$[A]$	$[B]$	Rate of reaction
$1$	$0.1$	$0.1$	$2 \times {10^{ - 3}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$
$2$	$0.4$	$0.1$	$0.4 \times {10^{ - 2}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$
$3$	$0.1$	$0.2$	$1.4 \times {10^{ - 2}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$

In the reaction, $A + B \to C + D$ , the rate $\left( {\frac{{dx}}{{dt}}} \right)$ when plotted against time $'t'$ gives a straight line parallel to time axis. The order and rate of reaction will be

What is the order of a reaction which has a rate expression rate $ = K{[A]^{3/2}}{[B]^{ - 1}}$

For a certain reaction, $10\%$ of the reactant dissociates in $1\, hour$, $20\%$ of the reactant dissociate in $2\, hour$, $30\%$ of the reactant dissociates in $3\, hour$. Then the units of rate constant is

Select the rate law for reaction $A + B \longrightarrow C$

What is the order of reaction' for $A + B \to C$