Consider the following data for the reaction: $A+BC+D$

$[$A$]($M$)$

The rate law is given by

$k[A{]}^2[B][D{]}^{-1}$

$k[A{]}^2[B{]}^{-1}[D{]}^{\frac{1}{2}}$

$k[A][B{]}^{\frac{1}{2}}[D{]}^{-\frac{1}{2}}$

$k[A{]}^{-1}[B][D{]}^{\frac{1}{2}}$

$k[A{]}^{-1}[B][D{]}^{-\frac{1}{2}}$

none of the above

The rate constant $k$ is equal to

$2\mathrm{.}5{10}^3$

$1\mathrm{.}8$

$36$

$1\mathrm{.}4{10}^4$

$4\mathrm{.}0{10}^5$

The correct units for the rate constant are

$M^{\frac{3}{2}}$min$-1$

$M^{\frac{1}{2}}$min$-1$

min$-1$

$M^{-\frac{1}{2}}$min$-1$

$M^{-1}$min$-1$