The following results have been obtained during the kinetic studies of the reaction: $2 \ NO + 2 \ H_2 \longrightarrow N_2 + 2 \ H_2O$

Expt	$\frac{-d[NO]}{dt} \ (mol \ L^{-1} \ s^{-1})$	$[NO] \ (mol \ L^{-1})$	$[H_2] \ (mol \ L^{-1})$
$1$	$4.8 \times 10^{-5}$	$1 \times 10^{-2}$	$1 \times 10^{-3}$
$2$	$43.2 \times 10^{-5}$	$3 \times 10^{-2}$	$1 \times 10^{-3}$
$3$	$86.4 \times 10^{-5}$	$3 \times 10^{-2}$	$2 \times 10^{-3}$

• A
  $\frac{-d[NO]}{dt} = k[NO]^2[H_2]$
• B
  $\frac{-d[NO]}{dt} = k[NO]^2[H_2]^{\frac{1}{2}}$
• C
  $\frac{-d[NO]}{dt} = k[NO][H_2]^2$
• D
  $\frac{-d[NO]}{dt} = k[NO][H_2]$