In the following reaction $A \to B + C$, rate constant is $0.001\, M/sec$. If we start with $1M$ of $A$, the conc. of $A$ & $B$ after $10$ min are respectively

The rate of reaction between $A$ and $B$ increases by a factor of  $100,$ when the concentration of $A$ is increased $10$ folds. The order of reaction with respect to $A$ is

The rate of the reaction :

$2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.

$\frac{-d[N_2O_5 ]}{dt} = k[N_2O_5]$

$\frac{d[NO_2 ]}{dt} = k'[N_2O_5]\,;$   $\frac{d[O_2 ]}{dt} = k"[N_2O_5]$

The relationship between $k$ and $k'$ and betweenk and $k''$ are

For which order reaction a straight line is obtained along with $x\,-$ axis by plotting a graph between half life $({t_{1/2}})$ and initial concentration $ 'a'$

Catalyst decomposition of hydrogen peroxide is a ........ order reaction

The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)$ and $(ii).$ The respective orders of the reactions are