Reaction $aA + bB\,\to $ product. The rate of reaction $= k[A]^3\, [B]^0$ if the concentration of $A$ is double and concentration of $B$ is half the rate will be ?

For conversion of compound $A \rightarrow B$, the rate constant of the reaction was found to be $4.6 \times 10^{-5}\,L\, mol ^{-1}\, s ^{-1}$. The order of the reaction is $..........$ 

For the reaction $2NO_2 + F_2 \to  2NO_2F$, following mechanism has been provided :
$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$
$N{O_2} + {F_2}\xrightarrow{{fast}}N{O_2}F$
Thus rate expression of the above reaction can be written as

The reaction ${N_2}{O_5}$ (in $CCl_4$ solution) $ \to 2N{O_2}$ (solution) $ + \frac{1}{2}{O_2}(g)$ is of first order in ${N_2}{O_5}$ with rate constant $6.2 \times {10^{ - 1}}{s^{ - 1}}.$ What is the value of rate of reaction when $[{N_2}{O_5}] = 1.25\,mole\,{l^{ - 1}}$

Assuming the reaction

$2NO(g) + Cl_2(g) \longrightarrow 2NOCl(g)$

occurs in a single elementary step, we can say that

Select the rate law for reaction $A + B \longrightarrow C$