The reaction
$$\ce{2 A + B + C -> D + 2 E}$$
is found to follow the rate law as
$$r = k[\ce{A}][\ce{B}]^2[\ce{C}]^0$$
If the concentration of $\ce{A}$, $\ce{B}$ and $\ce{C}$ increases two times then the rate of reaction becomes eight times higher:
$$r' = k\cdot 2[\ce{A}]\left(2[\ce{B}]\right)^2\left(2[\ce{C}]\right)^0 = 8k[\ce{A}][\ce{B}]^2$$
Note: there is no change in the order of reaction. I want to change the order of this reaction by changing the concentration of reactants. Can I do this?
Because if we double the concentration of $\ce{A}$, $\ce{B}$ or $\ce{C}$, it does not change the order. But if we increase the concentration of $\ce{A}$ by 4 times, then we can change order by
$$\left(4[\ce{A}]\right)^2 = \left(2[\ce{A}]\right)^{2+2} = \left(2[\ce{A}]\right)^4$$