Which one of the following statements for the order of a reaction is incorrect?

The rate of the reaction, 2NO + Cl₂ $$ \to $$ 2NOCl is given by the rate equation rate = k[NO]²[Cl₂]. The value of the rate constant can be increased by

For the reaction N₂O_5(g) $$ \to $$  2NO_2(g) + 1/2O_2(g)
the value of rate of disappearance of N₂O₅ is given as 6.25 $$ \times $$ 10^$$-$$3 mol L^$$-$$1 s^$$-$$1. The rate of formation of NO₂ and O₂ is given respectively as

During the kinetic study of the reaction, 2A + B $$ \to $$ C + D, following results were obtained

Run	[A]/mol L$$-$$1	[B]/mol L$$-$$1	Initial rate of formation of D/mol L$$-$$1 min$$-$$1
I.	0.1	0.1	6.0$$ \times $$10$$-$$3
II.	0.3	0.2	7.2$$ \times $$10$$-$$2
III.	0.3	0.4	2.88$$ \times $$10$$-$$1
IV.	0.4	0.1	2.40$$ \times $$10$$-$$2

Based on the above data which one of the following is correct?