Mechanism of a hypothetical reaction

$X_2 + Y_2 \rightarrow 2XY,$ is given below :

$(i)\,\, X_2 \rightarrow X + X\, (fast)$

$(ii)\,\,X + Y_2 \rightleftharpoons XY + Y\, (slow)$

$(iii)\,\,X + Y \rightarrow XY\, (fast)$

The overall order of the reaction will be

A student has studied the decomposition of a gas $AB _3$ at $25^{\circ} C$. He obtained the following data.

The order of the reaction is

The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:

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

For a reaction $A \to B$, the rate of reaction quadrupled when the concentration of $A$  is doubled. The rate expression of the reaction is $r = K{(A)^n}$. when the value of $n$ is

For reaction
$X_2(g) + Y_2(g) \rightarrow  2XY (g)$

The following data are observed

Rate constant of reaction will (in $M^{1-n}\,sec^{-1}$) where $'n'$ is order of reaction