The rate equation for the reaction $2\mathrm{A}+\mathrm{B}\to \mathrm{C}$ is found to be: $\text{ rate }=k\left[\mathrm{A}\right]\left[\mathrm{B}\right]$. The correct statement in relation to this reaction is that the 

For the reaction $2\mathrm{A}+\mathrm{B}\to \mathrm{C}$, the rate law is $r=k\left[\mathrm{A}\right]\left[\mathrm{B}\right]$

The unit of $k$ will be ${\mathrm{mol}}^{-1} \mathrm{L} {\mathrm{s}}^{-1}$. The half-life period, $t_{1/2}$ is not constant.

The rate of formation of C will be half of the rate of disappearance of A. The rate constant will be independent of initial concentrations of A and B.