Use the data to determine rate law for reaction: $2NO+H_2\rightarrow N_2O+H_2O$

Question

Experiment No	$[NO]$	$[H_2]$	Initial rate
1	0.021	0.065	1.46M/min
2	0.021	0.260	1.46M/min
3	0.042	0.065	5.84M/min

 

$\begin{array}{1 1}(a)\;R=K[NO][H_2]\\(B)\;R=K[NO]^2[H_2]\\(c)\;R=K[H_2]^2\\(d)\;R=K[NO]^2\end{array}$