The following results are obtained for the reaction $S + Nu \rightarrow \text{product}$. By which reaction mechanism does this reaction occur?

Experiment	$[S]$	$[Nu]$	Rate
$1$	$0.1$	$0.1$	$2.2 \times 10^{-3}$
$2$	$0.2$	$0.1$	$4.4 \times 10^{-3}$
$3$	$0.1$	$0.2$	$4.4 \times 10^{-3}$

The number of incorrect statement/s from the following is:
$A$. The successive half-lives of zero-order reactions decrease with time.
$B$. $A$ substance appearing as a reactant in the chemical equation may not affect the rate of reaction.
$C$. Order and molecularity of a chemical reaction can be a fractional number.
$D$. The rate constant units of zero and second-order reactions are $mol \ L^{-1} s^{-1}$ and $mol^{-1} L s^{-1}$ respectively.

If the rate constant $k = 4.5 \times 10^{-7} \text{ L}^2 \text{ mol}^{-2} \text{ s}^{-1}$,then what is the order of the reaction?

At $345 \ K$,the half-life for the decomposition of a sample of a gaseous compound initially at $55.5 \ kPa$ was $340 \ s$. When the pressure was $27.8 \ kPa$,the half-life was found to be $170 \ s$. The order of the reaction is $......$ [integer answer]

Write the general reaction,its differential rate equation,and the rate law.

For the reaction $A + 2B \to C$,the rate equation is given as $\text{Rate} = K[A][B]$. If the concentration of $A$ is kept constant but that of $B$ is doubled,what will happen to the rate of the reaction?