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 the reaction, $2N_2O_5 \to 4NO_2 + O_2$ rate and rate constant are $1.02 \times 10^{-4}\, mol\,L^{-1}\,s^{-1}$ and $3.4 \times10^{-5}\,s^{-1}$ respectively. The concentration of $N_2O_5$ in $mol\,L^{-1}$ will be

For a certain reaction the expression for half life is $t \propto \frac{1}{{{a^{n - 1}}}}$ then the order of reaction is

If $R = K{[NO]^2}[{O_2}],$ rate constant may be increased by

Write general equation of reaction and explain - what is order of reaction ? Which is its value ?

In a reaction, the concentration of reactant is increased two times and three times then the increases in rate of reaction were four times and nine times respectively, order of reaction is