Which of these does not influence the rate of reaction?

The unit of the rate constant depends on which of the following?

The reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism $A_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2A$ (fast),$A + B_2 \xrightarrow{k_2} AB + B$ (slow),$A + B \rightarrow AB$ (fast). The overall order of the reaction is:

The reaction of hydrogen and iodine monochloride is given as :
$H_{2(g)} + 2ICl_{(g)} \rightarrow 2HCl_{(g)} + I_{2(g)}$
This reaction is of first order with respect to $H_{2(g)}$ and $ICl_{(g)}$. The following mechanisms were proposed:
Mechanism $A$ :
$H_{2(g)} + 2ICl_{(g)} \rightarrow 2HCl_{(g)} + I_{2(g)}$
Mechanism $B$ :
$H_{2(g)} + ICl_{(g)} \rightarrow HCl_{(g)} + HI_{(g)}$ ; (slow)
$HI_{(g)} + ICl_{(g)} \rightarrow HCl_{(g)} + I_{2(g)}$ ; (fast)
Which of the above mechanism$(s)$ can be consistent with the given information about the reaction?

For a reaction,$A + 2B \longrightarrow C$,the rate is given by $+\frac{d[C]}{dt} = k[A][B]$. Hence,the order of the reaction is:

When the concentration of $A$ in the reaction $A + B \rightleftharpoons AB$ is doubled,the rate of reaction will be