Question

Table #1: Volumes

Trial	Deionized Water (mL)	1.0 M KI (mL)	H2O2 (mL)	Temperature of Tap Water (◦C)
1	100	50	50	18.7
2	125	25	50	19.3
3	125	50	50	19.5
4	100	50	50	50.0

Table #2: Trial #1 data

Time (min)	Volume (mL)	Time (min)	Volume (mL)
3	0	8	12
4	1	9	15
5	4	10	18
6	6	11	25
7	8	12	27

Table #3: Trial #2 data

Time (min)	Volume (mL)	Time (min)	Volume (mL)
6.27	0	11.27	6
7.27	1	12.27	7
8.27	3	13.27	9
9.27	4	14.27	11
10.27	6	15.27	12

Table #4: Trial #3 data

Time (min)	Volume (mL)	Time (min)	Volume (mL)
5.37	0	9.37	5
6.37	2	10.37	6
7.37	3	11.37	8
8.37	4	12.37	9

Table #5: Trial #4 data

Time (min)	Volume (mL)	Time (min)	Volume (mL)
1.30	0	6.30	62
2.30	5	7.30	82
3.30	13	8.30	100
4.30	26	9.30	115
5.30	41	10.30	132

Table #6: Results

Trial	Temperature (K)	3% H2O2 (M)	KI (M)	Rate (L/min)
1	291.85	0.176	0.005	0.00225
2	292.45	0.176	0.0025	0.00075
3	292.65	0.176	0.005	0.0009
4	323.15	0.176	0.005	0.0132

Above are 6 tables of data from an experiment I performed. My goal is to determine the reaction order with respect to H2O2 and I- , the rate law for the reaction, and the activation energy for the reaction. My first issue is table #6. I do not believe that I have figured the correct (M) for the H2O2 and KI or the correct rate. I am supposed to make sure to express the concentrations based on the values after dilution due to mixing. I am not sure how to correctly calculate that.