Consider the given plots for a reaction obeying Arrhenius equation (0^oC < T < 300^oC) : (K and Ea are rate constant and activation energy, respectively)



Choose the correct option :

For the reaction, 2A + B $$ \to $$ products, when the concentrations of A and B both were doubled, the rate of the reaction increased from 0.3 mol L^$$-$$1s^$$-$$1 to 2.4 mol L^$$-$$1s^$$-$$1. When the concentration of A alone is doubled, the rate increased from 0.3 mol L^$$-$$1s^$$-$$1 to 0.6 mol L^$$-$$1s^$$-$$1.

The following results were obtained during kinetic studies of the reaction ;
2A + B $$ \to $$ Products

Experiment	[A] (in mol L$$-$$1)	[b] (in mol L$$-$$1)	Initial Rate of reaction (In mol L$$-$$1 min$$-$$1)
I	0.10	0.20	6.93 G 10$$-$$3
II	0.10	0.25	6.93 G 10$$-$$3
III	0.20	0.30	1.386 G 10$$-$$2

The time (in minutes) required to consume half of A is :

If 50% of a reaction occurs in 100 second and 75% of the reaction occurs in 200 secod, the order of this reaction is :