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

In a reaction, the concentration of reactant is increased two times and three times then the increases in rate of reaction were four times and nine times respectively, order of reaction is

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

Assuming the reaction

$2NO(g) + Cl_2(g) \longrightarrow 2NOCl(g)$

occurs in a single elementary step, we can say that

The rate constant of the reaction $2H_2O_2(aq) \to  2H_2O(aq) + O_2(g)$ is $3\times10^{-3}\, min^{-1}$. At what concentration of $H_2O_2$, the rate of reaction will be $2\times10^{-4}\, M\, s^{-1}$ ? ............ $M$

For the reaction

$2 \mathrm{H}_{2}(\mathrm{g})+2 \mathrm{NO}(\mathrm{g}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$

the observed rate expression is, rate $=\mathrm{k}_{\mathrm{f}}[\mathrm{NO}]^{2}\left[\mathrm{H}_{2}\right] .$ The rate expression of the reverse reaction is