Velocity constant $K$ of a reaction is affected by

Which of the following rate laws has an overall order of $0.5$  for reaction involving substances $x$, $y$ and $z$

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)

The concentration of $R$ in the reaction $R \rightarrow P$ was measured as a function of time and the following data is obtained:

The order of the reaction is

For a reaction scheme. $A\xrightarrow{{{k_1}}}B\xrightarrow{{{k_2}}}C$ if the rate of formation of $B$ is set to be zero then the concentration of $B$ is given by

For a certain reaction, the rate $=k[A]^2[B]$, when the initial concentration of $A$ is tripled keeping concentration of $B$ constant, the initial rate would