You use 20. mL of a solution containing 6.0% H2O2 by mass (m/m).Assume the density of the solution is 1.0 g/mL and that all of thehydrogen peroxide decomposes according to the reaction:
2 H2O2 (aq) ? 2 H2O (l) + O2 (g)

A)How many total moles of oxygen gas can be generated through thisdecomposition?

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Using a 25.00 mL of 3.00% by mass solution ({mass H2O2/masssolution}*100) of hydrogen peroxide. Assume the density of thissolution is 1.000 g/mL. If all of the hydrogen peroxide decomposesto water and oxygen according to the reaction

2 H2O2 (aq) <----> 2 H2O (l) + O2 (g)

What is the total volume of oxygen gas generated if the temperatureis 24 degrees Celsius and the pressure is 770 Torr (760 Torr=1atm)? (R=0.08206 L*atm/K*mol) (At this point you can ignore theeffect of water vapor)

Any assistance would be great, its been awhile since I have had anychemistry and don't know how to approach this. I have an idea ofhow to do it, but I haven't done some of the simple stuff in a longtime like converting moles of H2O2 to moles of O2

The active ingredient in many hair bleaches is hydrogen peroxide, H2O2. The amount of hydrogen peroxide present can be determined by titration with a standard permanganate, MnO4, solution: 2 MnO4?(aq) + 5 H2O2(aq) + 6 H+(aq) ---> 5 O2 (g) + 2 Mn+2 (aq) + 8 H2O (l)Calculate the molarity of hydrogen peroxide if 28.75 mL of hydrogen peroxide produced 695 mL of oxygen gas at 0.950 atm and 315 K?

Redox titrations are used to determine the amounts of oxidizing andreducing agents in solution. For example, H2O2 a solution ofhydrogen peroxide, , can be titrated against a solution ofpotassium permanganate, KMnO4. The following equation representsthe reaction:

2KMnO4(aq) + H2O2(aq) + 3H2SO4 (aq) ---> O2(g) + 2MnSO4(aq) +K2SO4(aq) + 4H2O(l)

A certain amount of hydrogen peroxide was dissolved in 100 mL ofwater and then titrated with 1.68 M KMnO4. How much H2O2 wasdissolved if the titration required 22.3mL of the KMnO4solution?

mass of H2O2= ?

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You use 20. mL of a solution containing 6.0% H2O2 by mass (m/m).Assume the density of the solution is 1.0 g/mL and that all of thehydrogen peroxide decomposes according to the reaction:
2 H2O2 (aq) ? 2 H2O (l) + O2 (g)

A)How many total moles of oxygen gas can be generated through thisdecomposition?

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You use 20. mL of a solution containing 6.0% H2O2 by mass (m/m).Assume the density of the solution is 1.0 g/mL and that all of thehydrogen peroxide decomposes according to the reaction:2 H2O2 (aq) ? 2 H2O (l) + O2 (g)A)How many total moles of oxygen gas can be generated through thisdecomposition?

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

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Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

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