For the reaction $A + B \to$ products,doubling the concentration of $A$ the rate of the reaction is doubled,but on doubling the concentration of $B$ the rate remains unaltered. The overall order of the reaction is:

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

With the help of an example,explain what is meant by a pseudo first order reaction.

The numerical values of rate constants are same for first,second and third order reactions. Which one is true at a moment for rate of these three reactions if concentration of reactants is same and lesser than $1 \ M$?

Ozone decomposes into oxygen as follows:
$O_3 \rightleftharpoons O_2 + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction $2O_3 \to 3O_2$.

Which of the following statements is false?