The value of $\frac{t_{0.875}}{t_{0.50}}$ for $n^{th}$ order reaction is

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

The rate law equation for a reaction between $A$,$B$ and $C$ is $r = k[A][B][C]^2$. What will be the new rate of reaction if the concentration of both $A$ and $B$ are doubled (in $r$)?

$A$ complex reaction takes place in the following steps:
$NO_2Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{(g)}$ (slow)
$NO_2Cl_{(g)} + Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{2(g)}$ (fast)
Identify the rate law equation for this reaction.

$2 \ FeCl_3 + SnCl_2 \rightarrow 2 \ FeCl_2 + SnCl_4$. This reaction is an example of:

Match List-$I$ with List-$II$:

List-$I$ (Order of Reaction)	List-$II$ (Unit of rate constant)
$A$. Zero order	$I$. $mol^{-1} L s^{-1}$
$B$. First order	$II$. $mol^{-2} L^{2} s^{-1}$
$C$. Second order	$III$. $s^{-1}$
$D$. Third order	$IV$. $mol L^{-1} s^{-1}$