The catalytic decomposition of hydrogen peroxide can be expressed as: H2O2(aq) → H2O(l) + O2(g) What are the stoichiometric coefficients for the reaction above? (enter the coefficients without commas or spaces in between, e.g. 557) Calculate the number of moles of oxygen gas produced from the completely catalyzed decomposition of 6.00 mL sample of a 3.5% solution of H2O2. The density of the 3.5% solution of H2O2 is 1.01 g/mL. 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 280 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 catalytic decomposition of hydrogen peroxide can be expressed as:
H2O2(aq) → H2O(l) + O2(g)
What are the
Calculate the number of moles of oxygen gas produced from the completely catalyzed decomposition of 6.00 mL sample of a 3.5% solution of H2O2. The density of the 3.5% solution of H2O2 is 1.01 g/mL.
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 | 280 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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