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?

For the reaction, N₂ + 3H₂ $$ \to $$ 2NH₃, if
$${{d\left[ {N{H_3}} \right]} \over {dt}}$$ = 2 $$ \times $$ 10^$$-$$4 mol L^$$-$$1 s^$$-$$1,
the value of $${{ - d\left[ {{H_2}} \right]} \over {dt}}$$ would be

In the reaction,
BrO$$_{3(aq)}^ - $$ + 5Br$$_{(aq)}^ - $$ + 6H⁺ $$ \to $$ 3Br_2(l) + 3H₂O_(l).
The rate of appearance of bromine (Br₂) is related to rate of disappearance of bromide ions as

For the reaction A + B $$ \to $$ products, it is observed that

(i)  on doubling the initial concentration of A only, the rate of reaction is also doubled and
(ii)  on doubling the initial concentration of both A and B, there is a change by a factor of 8 in the rate of the reaction.

The rate of this reaction is given by