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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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.