Consider the reaction :

$Cl_2(aq) + H_2S(aq) \to  S(s) + 2H^+(aq) + 2Cl^-(aq)$

The rate equation for this reaction is rate $= k[Cl_2][H_2S]$ Which of these mechanisms is/are consistent with this rate equation ?

$A.\,C{l_2} + {H_2}S \to {H^ + } + C{l^ - } + C{l^ + } + H{S^- }$  (slow)

$C{l^ + } + H{S^ - } \to {H^ + } + C{l^ - } + {S}$   (fast)

$B.\, H_2S  \Leftrightarrow  H^+ + HS^-$   (fast equilibrium)

$Cl_2 + HS^-\to  2Cl^-+ H^+ + S$ (slow)

The decomposition of $NH _{3}$ on $Pt$ surface is a zero order reaction. If the value of rate constant is $2 \times 10^{-4}\,mole $ $liter^{-1}\, sec ^{-1}$ The rate of appearance of $N _{2}$ and $H _{2}$ are respectively.

 $A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$  but it is independent of the concentration of $B$, then

The reaction, $X + 2Y + Z \to N$ occurs by the following mechanism

$(i)$ $X + Y \rightleftharpoons M$      very rapid equilibrium

$(ii)$ $M + Z \to P$      slow

$(iii)$ $O + Y \to N$      very fast

What is the rate law for this reaction

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?

A student has studied the decomposition of a gas $AB _3$ at $25^{\circ} C$. He obtained the following data.

The order of the reaction is