🤓 Based on our data, we think this question is relevant for Professor Seitz's class at UNH.
First thing is to find the mass of H2O2 in the reactant. In this case, the solution (125 g) contains 50% H2O2 by weight so there will be 62.5 g of H2O2
(125 g) (0.5) = 62.5 g
We need to get the molar mass of H2O2 which will be used to find the moles of H2O2
Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe):
2H2O2(aq) → 2H2O(l) + O2(g)
What volume of pure O2(g), collected at 27°C and 746 torr, would be generated by decomposition of 125 g of a 50.0% by mass hydrogen peroxide solution? Ignore any water vapor that may be present.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.
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Based on our data, we think this problem is relevant for Professor Seitz's class at UNH.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.