The reaction, $X + 2Y + Z \to  N$ occurs by the following mechanism

$(i)$ $X + Y  \rightleftharpoons  M$             very rapid equilibrium

$(ii)$ $M + Z \to  P$                        slow

$(iii)$ $O + Y \to  N$                       very fast

What is the rate law for this reaction

For a reaction $A \to$ Products, a plot of $log\,t_{1/2}$ versus $log\,a_0$ is shown in the figure. If the initial concentration of $A$ is represented by $a_0,$ the order of the reaction is

Order of a reaction is decided by

Consider the data given below for hypothetical reaction $A \to X$

$Time  (sec)$                     Rate $(mol\,  L^{-1} sec.^{-1})$

$0$                                      $1.60 \times 10^{-2}$

$10$                                    $1.60 \times 10^{-2}$

$20$                                    $1.60 \times 10^{-2}$

$30$                                    $1.60 \times 10^{-2}$

From the above data, the order of reaction is

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

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.

$(ii)$ $H _{2} O _{2}( aq )+3 I ^{-}( aq )+2 H ^{+} \rightarrow 2 H _{2} O ( l )+ I _{3}^{-} \quad$ Rate $=k\left[ H _{2} O _{2}\right][ I ]$