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

If the rate constant $k = 4.5 \times 10^{-7} \text{ L}^2 \text{ mol}^{-2} \text{ s}^{-1}$, then what is the order of the reaction?

For the reaction $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. What is the concentration of $N_2O_5$?

Write the general reaction,its differential rate equation,and the rate law.

The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the

The number of incorrect statement/s from the following is:
$A$. The successive half-lives of zero-order reactions decrease with time.
$B$. $A$ substance appearing as a reactant in the chemical equation may not affect the rate of reaction.
$C$. Order and molecularity of a chemical reaction can be a fractional number.
$D$. The rate constant units of zero and second-order reactions are $mol \ L^{-1} s^{-1}$ and $mol^{-1} L s^{-1}$ respectively.