HELP !!!!!!!!! PLEASE HELP ME ON THE DARK BULLET POINT TABLE CALCULATION. BE SURE UPLOAD THE GRAPH. make sure Answer all of them
Experiment 1
Exact concentration of H2O2 stock solution (M)
1.014
Temperature of water bath (°C)
24
Experiment 1: Volume of O2 vs time for decomposition of H2O2
| Time (min) | |
|---|---|
| Volume of O2 (mL) 2.0 |
0.00 |
| 4 | 1.22 |
| 6 | 2.41 |
| 8 | 3.64 |
| 10 | 4.93 |
| 12 | 6.34 |
| 14 | 7.78 |
| 16 | 9.49 |
| 18 | 10.99 |
| 20 | 12.35 |
| 22 | 14.64 |
| 24 | 16.31 |
| 26 | 19.16 |
| 28 | 20.97 |
| 30 | 24.52 |
| 32 | 26.03 |
| 34 | 28.99 |
| 36 | 32.30 |
| 38 | 35.17 |
| 40 | 38.83 |
| 42 | 44.83 |
| 44 | 50.50 |
| 46 | 58.26 |
| 48 | 63.46 |
Experiment 2: Volume of O2 vs time for decomposition of H2O2
| Time (min) | |
|---|---|
| Volume of O2 (mL) 2.0 |
0.00 |
| 4 | 0.63 |
| 6 | 1.31 |
| 8 | 1.96 |
| 10 | 2.42 |
| 12 | 2.93 |
| 14 | 3.56 |
.
Experiment 3: Volume of O2 vs time for decomposition of H2O2
| Time (min) | |
|---|---|
| Volume of O2 (mL) 2.0 |
0.00 |
| 4 | 0.45 |
| 6 | 0.88 |
| 8 | 1.44 |
| 10 | 2.29 |
| 12 | 2.92 |
| 14 | 3.51 |
Calculations
For all three experiments plot the volume of O2 evolved in mL (on the y-axis) versus time in minutes (on the x-axis). Clearly label each experiment's plot and/or use a different color for each. Determine each initial
Experiment 1
What is the last point that you will use to determine the initial rate?
Choose...4.0 mL6.0 mL8.0 mL10.0 mL12.0 mL14.0 mL16.0 mL18.0 mL20.0 mL22.0 mL24.0 mL26.0 mL28.0 mL30.0 mL32.0 mL34.0 mL36.0 mL38.0 mL40.0 mL42.0 mL44.0 mL46.0 mL48.0 mL
Slope of tangent line for experiment 1:
Experiment 2
What is the last point that you will use to determine the initial rate?
Choose...4.0 mL6.0 mL8.0 mL10.0 mL12.0 mL14.0 mL
Slope of tangent line for experiment 2:
Experiment 3
What is the last point that you will use to determine the initial rate?
Choose...4.0 mL6.0 mL8.0 mL10.0 mL12.0 mL14.0 mL
Slope of tangent line for experiment 3:
Upload the graph(s) of your data here. Make sure each plot is properly labeled (axes defined, units labeled, titled properly). You can plot all three experiments on one graph, or split into three graphs.
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Concentration of H2O2 stock solution: 1.014 M
Concentration of KI stock solution: 0.10 M
Orders of reaction and specific rate constant
Table view
List view
Orders of reaction and specific rate constant
| Experiment 1 | Experiment 2 | Experiment 3 | |
|---|---|---|---|
| Initial molarity of H2O2 after dilution (M) | |||
| Initial molarity of I- after dilution (M) | |||
| Initial rate of reaction (mL O2/min) (slope of tangent determined above) |
|||
| Order of reaction with respect to H2O2 (estimated) |
--------- (blank) |
→
|
|
| Order of reaction with respect to I- (estimated) |
--------- (blank) |
→
|
|
| Order of reaction with respect to H2O2 (calculated) | |||
| Order of reaction with respect to I- (calculated) | |||
| Specific rate constant (using the calculated reaction order) |
|||
| Average specific rate constant |
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