The last part of this question. The catalytic decomposition of hydrogen peroxide can be expressed as: 2H2O2(aq) → 2H2O(l) + O2(g) Calculate the number of moles of oxygen gas produced from the completely catalyzed decomposition of 6.60 mL sample of a 3.5% solution of H2O2. The density of the 3.5% solution of H2O2 is 1.01 g/mL. 0.00343 A trial of this decomposition experiment, using different quantities of reactants than those listed in the question above produced the following data: Volume of O2 produced at room conditions 200 mL Barometric pressure 740 torr Temperature of water 24°C Termperature of O2 25°C Vapor Pressure due to water at 25°C 22.4 torr For the conditions listed above, calculate the volume of O2(g) produced at standard conditions of temperature and pressure. (enter your answer in liters)
The last part of this question. The catalytic decomposition of hydrogen peroxide can be expressed as: 2H2O2(aq) → 2H2O(l) + O2(g) Calculate the number of moles of oxygen gas produced from the completely catalyzed decomposition of 6.60 mL sample of a 3.5% solution of H2O2. The density of the 3.5% solution of H2O2 is 1.01 g/mL. 0.00343 A trial of this decomposition experiment, using different quantities of reactants than those listed in the question above produced the following data: Volume of O2 produced at room conditions 200 mL Barometric pressure 740 torr Temperature of water 24°C Termperature of O2 25°C Vapor Pressure due to water at 25°C 22.4 torr For the conditions listed above, calculate the volume of O2(g) produced at standard conditions of temperature and pressure. (enter your answer in liters)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The last part of this question.
The catalytic decomposition of hydrogen peroxide can be expressed as:
2H2O2(aq) → 2H2O(l) + O2(g)
Calculate the number of moles of oxygen gas produced from the completely catalyzed decomposition of 6.60 mL sample of a 3.5% solution of H2O2. The density of the 3.5% solution of H2O2 is 1.01 g/mL.
0.00343
A trial of this decomposition experiment, using different quantities of reactants than those listed in the question above produced the following data:
| Volume of O2 produced at room conditions | 200 mL |
| Barometric pressure | 740 torr |
| Temperature of water | 24°C |
| Termperature of O2 | 25°C |
| Vapor Pressure due to water at 25°C | 22.4 torr |
For the conditions listed above, calculate the volume of O2(g) produced at standard conditions of temperature and pressure. (enter your answer in liters)
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