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

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:

The rate of certain reaction depends on concentration according to the equation $\frac{{ - dc}}{{dt}} = \frac{{{K_1}C}}{{1 + {K_2}C}},$ what is the order, when concentration $(c)$ is very-very high

The mechanism for the reaction is given below $2P + Q \to S + T$ $P + Q \to R + S$(slow)$P + R \to T$ (fast)The rate law expression for the reaction is

The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is

For the reaction between $A$ and $B$ , the initial rate of reaction $(r_0)$ was measured for different initial concentration of $A$ and $B$ as given below Order of the reaction with respect to $A$ and $B$ respectively, is $\sqrt 2  = 1.4 ,\,\sqrt 3  \times 10^{-4}$