Consider the given plot of enthalpy of the following reaction between A and B.
A+ B $$ \to $$ C + D
Identify the incorrect statement.

The given plots represent the variation of the concentration of a reactant R with time for two different reactions (i) and (ii). The respective orders of the reactions are :

For a reaction scheme $$A\buildrel {{k_1}} \over \longrightarrow B\buildrel {{k_2}} \over \longrightarrow C$$,

if the rate of formation of B is set to be zero then the concentration of B is given by :

For the reaction 2A + B $$ \to $$ C, the values of initial rate at diffrent reactant concentrations are given in the table below. The rate law for the reaction is :

[A] (mol L-1)	[B] (mol L-1)	Initial Rate (mol L-1s-1)
0.05	0.05	0.045
0.10	0.05	0.090
0.20	0.10	0.72