The rate constant k, for the reaction ${N_2}{O_5}(g) \to $ $2N{O_2}(g) + \frac{1}{2}{0_2}(g)$ is $2.3 \times {10^{ - 2}}\,{s^{ - 1}}$. Which equation given below describes the change of $[{N_2}{O_5}]$ with time? ${[{N_2}{O_5}]_0}$ and ${[{N_2}{O_5}]_t}$ correspond to concentration of ${N_2}{O_5}$ initially and at time $t$.

The rate of reaction $A + 2B \to 3C$ becomes $72\, times$ when concentration of $A$ is tripled and concentration of $B$ is doubled then the order of reaction with respect to $A$ and $B$ respectively is

The order of the reaction occurring by following mechanism should be

$(i)$ ${A_2} \to A + A$ (fast)

$(ii)$ $A + {B_2} \to AB + B$ (slow)

$(iii)$ $A + B \to $ (fast)

In a reaction $A_2B_3(g) \to A_2(g) + \frac{3}{2}B_2(g)$, the pressure increases from $60$ torr to $75$  torr in $2.5\, minutes$. The rate of disappearance of $A_2B_3$ is ........ $torr\, min^{-1}$

The rate law of the reaction $A + 2B \to $Product is given by $\frac{{d[dB]}}{{dt}} = k[{B^2}]$. If $ A$  is taken in excess, the order of the reaction will be

Order of radioactive disintegration reaction is