During the kinetic study of the reaction, 2A B 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 10 x II 0.3 0.2 7.2 10 x III 0.3 0.4 2.88 x10–1 IV 0.4 0.1 2.40 10 x Based on the above data which one of the following is correct? (AIPMT 2010)

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 Rate = k[A][B]2