[zerality]

Hi I am stuck on this problem and would appreciate any availabel assistance.

For reaction: 2H2(g) + 2NO (g)  ---->  N2 (g) + 2H2O(g) the followig data was taken
Experiment 1: [NO]iniial = 10.0M
Experiment 2: [NO]intial = 20.0M
 
t(s)                     Experiment 1 [H2] in M                    Experiment 2 [H2] in M
0                         10 x 10^-3                                         10 x 10 ^-3
10                        8.4 x 10^-3                                        5.0 x 10 ^-3
20                         7.1 x 10^-3                                       2.5 x 10^-3
30                        not measured                                     1.3 x 10^-3
40                         5.0 x 10^-3                                         .63 x 10^-3
 
Determine kinetic order in [H2] and [N2]
 
Calculate the [H2] at 30 s

I know the kinetic order for [H2] is 1
I know the rate law = k' [H2]  and that k' = k [NO] ^n
I'm not sure what the kinetic order for [NO] is.  I know the [NO] initial was doubled from exp 1 to exp 2.

If I use t1/2 = .693/k , I find that k = .693/40 = .017325


Thanks