In the sequence of reaction $A$ $\xrightarrow{k_1} X$ $\xrightarrow{k_2} Y$ $\xrightarrow{k_3} Z$ with $k_3 > k_2 > k_1$,then the rate determining step is

Higher order $(>3)$ reactions are rare due to

For the first order decomposition reaction of $N_2O_5$,it is found that -
$(a)$ $2N_2O_5 \rightarrow 4NO_{2(g)} + O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$(b)$ $N_2O_5 \rightarrow 2NO_{2(g)} + 1/2 O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k'[N_2O_5]$
Which of the following is true?

If $a$ is the initial concentration of the reactant,the half-life period of the reaction of $n^{th}$ order is inversely proportional to

The rate of the reaction $x + y \rightarrow \text{product}$ is $5.4 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[x] = 0.2 \ mol \ dm^{-3}$ and $[y] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if it is first order in $X$ and second order in $Y$.

For the reaction $A \to B$,the rate increases by a factor of $2.25$ when the concentration of $A$ is increased by $1.5$. What is the order of the reaction?