Select the incorrect option :

For a reaction $r = k[A][B]^2$,if the concentration of $A$ is doubled,the rate of reaction:

The rate law for the reaction $A + 2B \rightarrow C + 2D$ is given by:

In the reaction $A + B \to \text{Products}$,if $B$ is taken in excess,then it is an example of

For the reaction $Cl_{2(aq)} + H_2S_{(aq)} \to S_{(s)} + 2H^+_{(aq)} + 2Cl^-_{(aq)}$, the rate law is given by $\text{Rate} = K[Cl_2][H_2S]$. Which of the following mechanisms is consistent with this rate law?
$(A)$ $Cl_2 + H_2S \to H^+ + Cl^- + Cl^+ + HS^-$ (slow); $Cl^+ + HS^- \to H^+ + Cl^- + S$ (fast)
$(B)$ $H_2S \rightleftharpoons H^+ + HS^-$ (fast equilibrium); $Cl_2 + HS^- \to 2Cl^- + H^+ + S$ (slow)

Rate of the reaction $A + B \rightarrow \text{product}$ is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ and rate law is $r = k[A][B]^2$. What is the rate constant of the reaction if $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$?