During the kinetic study of the reaction, $\text{2A\hspace{0.17em}+\hspace{0.17em}B\hspace{0.17em}}\to \text{\hspace{0.17em}C\hspace{0.17em}+\hspace{0.17em}D}$, following results were obtained: 

 

 

 

 

 

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

In case of (II) and (III), keeping concentration of [A] constant, when the concentration of [B] is doubled, the rate quadruples. Hence it is second order with respect to B. in case of I & IV keeping the concentration of [B] constant. When the concentration of [A] is increased four times, rate also increases four times. Hence, the order with respect to A is one, hence $\text{Rate\hspace{0.17em}=\hspace{0.17em}k\hspace{0.17em}}\left[\text{A}\right]{\left[\text{B}\right]}^{\text{2}}$