The following data was obtained for chemical reaction given below at $975\, \mathrm{~K}$.

$2 \mathrm{NO}_{(\mathrm{g})}+2 \mathrm{H}_{2(\mathrm{~g})} \rightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})}$

	$[NO]$ $\mathrm{mol} \mathrm{L}^{-1}$	${H}_{2}$ $\mathrm{mol} \mathrm{L}^{-1}$	Rate  $\mathrm{mol}L^{-1}$ $s^{-1}$
$(A)$	$8 \times 10^{-5}$	$8 \times 10^{-5}$	$7 \times 10^{-9}$
$(B)$	$24 \times 10^{-5}$	$8 \times 10^{-5}$	$2.1 \times 10^{-8}$
$(C)$	$24 \times 10^{-5}$	$32 \times 10^{-5}$	$8.4 \times 10^{-8}$

The order of the reaction with respect to $\mathrm{NO}$ is ..... .

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.

$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$

The following data is given for reaction between $A$ and $B$

  Which of the following are correct statements -

$(a)$  Rate constant of the reaction $10^{-4}$

$(b)$  Rate law of the reaction is $k[A][B]$

$(c)$  Rate of reaction increases four times on doubling the concentration of both the reactant

For $n^{th}$ order reaction where $(n < 1)$

The reaction, ${N_2}{O_5} \longrightarrow 2NO + \frac{1}{2}\,{O_2}$ is of first order for $N_2O_5$ with rate constant $6.2 \times 10^{-4}\, s^{-1}$. what is the value of rate of reaction when $[N_2O_5] = 1.25\, mol\, L^{-1}$

Which among the following is a false statement