Question

Using The Following Data, Determine the Rate Law For The Reaction.

Part A.

2NO(g)+O(g) --> 2NO2(g)

Experiment	[NO]	[O2]	Initial Rate (M/s]
1	0.0126	0.0125	1.41x10^-2
2	0.0252	0.0250	1.13x10^-1
3	0.0252	0.0125	5.64x10^-2

Part B.

S2O8charge2-(ag)+3 I charge 1-(aq) ----> 2SO4charge2-(aq)+I3charge1-(aq)

Experiment	[S2O8charge2-]	[ I charge1-]	Initial Rate (M/s)
1	0.023	0.048	6.8x10^-6
2	0.054	0.048	1.6x10^-5
3	0.054	0.019	6.3x10^-6

Answer 1

Part A

from the table one while moving from first column to last column

if concentration No doubles rate increased two times that means wrt to NO second order

simlarly while moving from third column to second column concentration od O2 doubles rate become doubled so wrt O2 it is first order

rate law

rate = k [NO]² [O2]¹

second part is little confusing plaz ask somebady