CHG 3331 Lecture 5: Tutorial 7 Equations
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Table #1: Volumes
Trial | Deionized Water (mL) | 1.0 M KI (mL) | H2O2 (mL) | Temperature of Tap Water (â¦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.