2NO(g) + O2(g) → 2NO2(g)
Series of experiments are conducted by keeping the concentration of one of the reactants as constant and changing the concentration of the others.
Rate = k [NO]m [O2]n
For experiment 1, the rate law is
Rate1 = k [NO]m[O2]n
19.26 x 10-2 = k [1.3]m [1.1]n ……….(1)
For experiment 2
Rate2 = k [NO]m [O2]n
38.40 x 10-2 = k [1.3]m[2.2]n …….(2)
For experiment 3
Rate3 = k [NO]m [O2]n
76.8 x 10-2 = k [2.6]m[1.1]n ……(3)
Therefore the reaction is first order with respect to O2
Therefore the reaction is second order with respect to NO
The rate law is Rate = k [NO]2[O2]1
The overall order of the reaction = 2 + 1 = 3