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

The reaction is first order in A and first order in B, according to the rate equation rate = k[A][B]. In light of this, the reaction's overall order is 2.
(A) The concentration of A and B at the start has no effect on the value of k. Consequently, assertion B is true.
(B) The half-life time is variable. It varies inversely with the concentration of the reactants. Therefore, statement B is untrue.
(C) The rate of production of C is half that of A's rate of extinction.

$\frac{\mathrm{d}\left[\mathrm{C}\right]}{\mathrm{dt}}=\frac{-\mathrm{d}\left[\mathrm{A}\right]}{2\mathrm{dt}}$