For the reaction $A + B \to $ products, what will be the order of reaction with respect to $A$ and $B$ ?

Exp.	$[A]\,(mol\,L^{-1})$	$[B]\,(mol\,L^{-1})$	Initial rate    $(mol\,L^{-1}\,s^{-1})$
$1.$	$2.5\times 10^{-4}$	$3\times 10^{-5}$	$5\times 10^{-4}$
$2.$	$5\times 10^{-4}$	$6\times 10^{-5}$	$4\times 10^{-3}$
$3.$	$1\times 10^{-3}$	$6\times 10^{-5}$	$1.6\times 10^{-2}$

For the reaction $A \to B$, the rate increases by a factor of $2.25 $ when the concentration of $A$ is increased by $ 1.5$. What is the order of the reaction

For the non-stoichiometric reaction $2A + B \to C + D,$ the following kinetic data were  obtained in three separate experiments, all at $298\,K$.

For the reaction the rate of formation of $C$ will be

For the decomposition of azoisopropane to hexane and nitrogen at $543$ $K ,$ the following data are obtained.

Calculate the rate constant.

Consider the reaction :

$Cl_2(aq) + H_2S(aq) \to  S(s) + 2H^+(aq) + 2Cl^-(aq)$

The rate equation for this reaction is rate $= k[Cl_2][H_2S]$ Which of these mechanisms is/are consistent with this rate equation ?

$A.\,C{l_2} + {H_2}S \to {H^ + } + C{l^ - } + C{l^ + } + H{S^- }$  (slow)

$C{l^ + } + H{S^ - } \to {H^ + } + C{l^ - } + {S}$   (fast)

$B.\, H_2S  \Leftrightarrow  H^+ + HS^-$   (fast equilibrium)

$Cl_2 + HS^-\to  2Cl^-+ H^+ + S$ (slow)

Write unit of rate constant of following reaction :

$1.$ fourth order

$2.$ third order