A + B + C Y (note the reaction is not balanced)

Trial	[A] (mol/L)	[B] (mol/L)	[C] (mol/L)	Rate (molL-1s-1)
1	0.0020	0.0020	0.0040	4.48x10-6
2	0.0020	0.0040	0.0040	4.48 x10-6
3	0.0020	0.0060	0.0040	4.48 x10-6
4	0.0020	0.0080	0.0040	4.48 x10-6
5	0.0040	0.0080	0.0040	1.79 x10-5
6	0.0060	0.0080	0.0040	4.03 x10-5
7	0.0060	0.0080	0.0010	1.01 x10-5
8	0.0060	0.0080	0.0020	2.02 x10-5
9	0.0060	0.0080	0.0030	3.02 x10-5

Rate = k[A]2[B]0[C]1

. What will most likely happen to the rate constant k if the temperature of the reaction was increased by 10oC?

6. A chemist proposed a mechanism for this reaction.

Step 1: 2A + C A2C (slow)

Step 2: A2C + B F (fast)

Step 3: F + C Y___________(very fast)

Net:

a) Cancel terms and write the overall (net) reaction.

b) Is this reaction mechanism supported by the empirical evidence? Why or why not.