Identify the order of the following reaction: $2 NO_{2(g)} \longrightarrow 2 NO_{(g)} + O_{2(g)}$

At what concentration of the reactant (in $M$) are the rate constants for first-order,second-order,and third-order reactions equal?

The rate of the reaction $2A + 3B \rightarrow 2C + D$ is $6 \times 10^{-4} \text{ mol dm}^{-3} \text{ s}^{-1}$, when $[A] = [B] = 0.3 \text{ mol dm}^{-3}$. If the reaction is of first order with respect to $A$ and zeroth order with respect to $B$, find the rate constant $k$.

For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate equation can be expressed in two ways $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$ and $+\frac{d[NO_2]}{dt} = k'[N_2O_5]$. $k$ and $k'$ are related as:

If the value of the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$,then identify the reaction order:

Which is the unit of the rate constant for a second-order reaction?