Identify the reaction order from each of the following rate constants.

$(i)$ $k=2.3 \times 10^{-5} \,L \,mol ^{-1}\, s ^{-1}$

$(ii)$ $k=3 \times 10^{-4}\, s ^{-1}$

Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$

Which is True $(T)$ and False $(F)$ in the following sentence ?

The order of this reaction is $2$.

Which of these does not influence the rate of reaction

The order of a reaction which has the rate expression $\frac{{dc}}{{dt}} = K{[E]^{3/2}}{[D]^{3/2}}$ is

For a reaction taking place in three steps at same temperature, overall rate constant $\mathrm{K}=\frac{\mathrm{K}_1 \mathrm{~K}_2}{\mathrm{~K}_3}$. If $\mathrm{Ea}_1, \mathrm{Ea}_2$ and $\mathrm{Ea}_3$ are $40$,$50$ and $60 \mathrm{~kJ} / \mathrm{mol}$ respectively, the overall $\mathrm{Ea}$ is ________ $\mathrm{kJ} / \mathrm{mol}$.

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