For the following reaction: $NO_2(g) + CO(g) \to NO(g) + CO_2(g)$, the rate law is: Rate $= k \,[NO_2]^2$. If $0.1\,mole$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?

The order of a reaction which has the rate expression $\frac{{dc}}{{dt}} = K{[E]^{3/2}}{[D]^{3/2}}$ is

For a reaction of order $\mathrm{n}$, the unit of the rate constant 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

In a reaction, $A + B \rightarrow$ product, rate is doubled when the concentration of $B$ is doubled, and rate increases by a factor of $8$ when the concentration of both the reactants $(A$ and $B)$ are doubled, rate law for the reaction can be written as

For a reaction, $A+B \rightarrow$ Product; the rate law is given by, $r=k[ A ]^{1 / 2}[ B ]^{2}$ What is the order of the reaction?