Question

At a certain temperature the following data were collected for thereaction:
4 NO2(g) + O2(g) --------> 2 N2O5(g)

[NO2](M) [O2](M) Initial rate (M/s)
0.0250 0.0110 3.10*10^-4
0.0250 0.0220 6.20*10^-4
0.0500 0.0110 6.20*10^-4


What is the rate law for this reaction?

a) rate = k[NO2][O2]

b) rate = k[NO2]2[O2]2

c) rate = k[NO2]

d) rate = k[NO2]0.5[O2]

What is the value of the rate constant for the reaction?
_________________L•mol-1•s-1 ?