Determining reaction order : Rate Laws(Chemistry)
The reaction of nitric oxide with hydrogen at 1280C is as follows:
2NO(g) +2H2 (g) -> N2(g) + 2H2O(g)
From the following experimental data, determine the rate law and the rate constant.
30 POINTS!

The order of the reaction is 4.

The rate law of the reaction will be :

Rate constant of the reaction: k =

Explanation:

Let the stoichiometric coefficient of the NO and in rate law be x and y .

Rate of the reaction is given  by :

1) When ,

R =  0.00600 M/s

..[1]

2) When ,

R =  0.144 M/s

..[2]

3) When ,

R =  0.0120 M/s

..[3]

Dividing [1] and [3]

y = 1

Dividing [1] and [2]

x = 3

The order of the reaction = x + y = 3 + 1 = 4

The rate law of the reaction will be :

Rate constant of the reaction: k

When ,

R =  0.00600 M/s

..[1]

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer