(1)
From experiments (1) and (2), [H2] is kept constant at 0.40 M and [NO] is doubled from 0.40 M to 0.80 M. The rate of the reaction is quadrupled from 4.6×10−3 M/s to 18.4×10−3 M/s. This suggests that the order of the reaction with respect to NO is 2.
From experiments (1) and (3), [NO] is kept constant at 0.40 M and [H2] is doubled from 0.40 M to 0.80 M. The rate of the reaction is doubled from 4.6×10−3 M/s to 9.2×10−3 M/s. This suggests that the order of the reaction with respect to H2 is 1.
The overall order of the reaction is 2+1=3.
(2)
The rate law expression is
rate =k[NO]2[H2]
(3)
To calculate the value of the rate constant (k), substitute the data for experiment (1) in the rate law expression.
rate 4.6×10−3=k[0.40]2×0.40
k=0.072mol−2L2s−1