Calculate the following for each run: the initial molarities of I- and H2O2 (from the solutions tables) the rates of reaction [I2]/time (calculate the [I2] from [S2O32-] and the reaction: I2(aq) + 2 S2O32-(aq) → 2I-(aq) + S4O62-(aq) Choose the correct rate law for this reaction from your calculations.
Calculate the following for each run: the initial molarities of I- and H2O2 (from the solutions tables) the rates of reaction [I2]/time (calculate the [I2] from [S2O32-] and the reaction: I2(aq) + 2 S2O32-(aq) → 2I-(aq) + S4O62-(aq) Choose the correct rate law for this reaction from your calculations.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter10: Fuels, Organic Chemicals, And Polymers
Section: Chapter Questions
Problem 119QRT
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Question
Given the following:
| Solutions | Flask 1 | Flask 2 | Flask 3 |
| 0.04 M KI | 25.0 mL | 25.0 mL | 12.5 mL |
| 1% starch | 5.00mL | 5.00mL | 5.00mL |
| 0.03 M Na2S2O3 | 5.50 mL | 5.50 mL | 5.50 mL |
| 0.05 M H2SO4 | 5.00 mL | 5.00mL | 5.00mL |
| 0.08 M NaCl | 0 | 0 | 10.0 mL |
and
| Solutions | Beaker 1 | Beaker 2 | Beaker 3 |
| 0.04 M H2O2 | 25.0 mL | 12.5 mL | 25.0 mL |
| deioinized water | 0 | 12.5 mL | 0 |
Following the procedure Run 1 is when Beaker 1 is added to Flask 1 and the timer is started giving the time recorded for the run in the table below. This is repeated with Beaker 2 and Flask 2 for Run 2 and finally Beaker 3 and Flask 3 for Run 3:
The results for these runs are given below:
| Run | Time (seconds) |
| 1 | 35 |
| 2 | 66 |
| 3 | 72 |
Calculate the following for each run:
- the initial molarities of I- and H2O2 (from the solutions tables)
- the
rates of reaction [I2]/time (calculate the [I2] from [S2O32-] and the reaction:
I2(aq) + 2 S2O32-(aq) → 2I-(aq) + S4O62-(aq)
Choose the correct rate law for this reaction from your calculations.
Group of answer choices
Rate=k[I-][H2O2]
Rate=k{I-]2[H2O2]
Rate=k[I-][H2O2]2
Rate=k[I-]2[H2O2]2
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