Fill up the blank :

$1.$ The rate of zero order reaction depends on ........... concentration of reactant.

$2.$ The molecularity of slow step is equal to ........... of overall reaction

$3.$ Rate  $=$ ........ $[A]^x$ $[B]^y$

Order of a reaction is decided by

For reaction

$Cl_2(aq) + H_2S(aq) \to S(s) + 2H^+(aq) + 2Cl^-(aq)$ rate law is $r = K[Cl_2][H_2S]$
then which of these mechanism 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)

For the following reaction: $NO_2(g) + CO(g) \to NO(g) + CO_2(g)$, the rate law is: Rate $= k \,[NO_2]^2$. If $0.1\,mole$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?

The rate law for a reaction between the substances $ A $ and $B$  is given by, rate $= k{[A]^n}{[B]^m}$. On doubling the concentration of $A$ and halving the concentration of $B$, the ratio of the new rate to the earlier rate of the reaction will be as

The rate of dissappearance of $MnO_4^-$ in the following reaction is $4.56 \times 10^{-3}\, M/s$

$2MnO_4^-+ 10I^-+ 16H^+ \to 2Mn^{2+} + 5I_2 + 8 H_2O$

The rate of apperance of $I_2$ is