Rate law and order

2010 AIPMT-PRE 1 question

1. 1 Chemical Kinetics
   During the kinetic study of the reaction $2A + B \rightarrow C + D$, following results were obtained:
   Run I: [A] = 0.1 mol $L^{-1}$, [B] = 0.1 mol $L^{-1}$, initial rate of formation of D = $6.0\times10^{-3}$ mol $L^{-1}min^{-1}$
   Run II: [A] = 0.3, [B] = 0.2, rate = $7.2\times10^{-2}$
   Run III: [A] = 0.3, [B] = 0.4, rate = $2.88\times10^{-1}$
   Run IV: [A] = 0.4, [B] = 0.1, rate = $2.40\times10^{-2}$
   Based on the above data which one of the following is correct?
   A rate = $k[A][B]^2$ B rate = $k[A]^2[B]$ C rate = $k[A][B]$ D rate = $k[A]^2[B]^2$
   Check Answer