please i need help with this quetions with steps?

Question

1.     The data in the table below is collected for the reaction: 

CO(g) + Cl₂(g) → COCl₂(g).  

a) Determine the rate law. _______________________________

b) Calculate the value of the rate constant k.   _________________

       

[CO]o (M)	[Cl2]o (M)	Initial Rate (M/s)
0.25	0.40	0.696
0.50	0.80	3.94
0.25	0.80	1.97

Answer 1

Comparing experiment 3 to 2, [CO] is doubled from 0.25 to 0.50 while [Cl₂] remains constant at 0.80. The rate goes from 1.97 to 3.94, i.e. it doubles. This tells us that the reaction is 1st order in CO. Next, we compare experiment 1 to 3 where [CO] is constant and [Cl₂] is doubled from 0.40 to 0.80. The rate goes from 0.606 to 1.97, i.e. it increases 2.8 fold (almost 3 fold). This would equate to a 1.6 order (less than 2nd order and greater than 1st order)

rate = k[CO][Cl₂]^1.6

0.696 M/s = k [0.25 M][0.40 M]^1.6

0.696 M/s = 0.0677 k

k = 10.3 M^-1.6s^-1

NOTE: This is a strange question since usually they give you even numbers for the order of the reaction. The observation that the order is 1.6 with respect to Cl₂ makes me think there may be an error in the data.