The value of rate constant of a pseudo-first-order reaction

In the following reaction, which of the following are not the correct expressions regarding how the rate of appearance of the product is related to the disappearance of the reactant?

${\mathrm{BrO}}_3^{-} \left(\mathrm{aq}\right)+5{\mathrm{Br}}^{-} \left(\mathrm{aq}\right)+6{\mathrm{H}}^{+} \left(\mathrm{aq}\right)⟶3{\mathrm{Br}}_2 \left(\mathrm{l}\right)+3{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

$\mathrm{A}+\mathrm{B}\to \mathrm{C}$

Rate is expressed in $\mathrm{mol} {\mathrm{L}}^{-1}{\min }^{-1}$

Select the incorrect options regarding the order.

For the chemical reaction,

$\mathrm{A}+\mathrm{B}+\mathrm{C}\to \mathrm{E}$

The rate of reaction is doubled when the concentration of $\mathrm{B}$ is doubled, and when the concentration of both $\mathrm{A}$ and $\mathrm{B}$ is doubled, the rate becomes doubled and when the concentration of both $\mathrm{B}$ and $\mathrm{C}$ are doubled the rate becomes quadrupled.

Which of the given statement(s) is/are correct?

For a 1^st order reaction:

$2{\mathrm{N}}_2{\mathrm{O}}_5 \left(\mathrm{g}\right)\to 4{\mathrm{NO}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)$