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Ideal Gas Law and Aqueous Hydrogen Peroxide

A 100.0 gram sample of aqueous hydrogen peroxide decomposes over time to make 3.31 L of O2(g) at 21 degrees Celsius and 715 Torr. What must the mass percentage of H2O2 is the solution? (Ignore the VP of H2O).

2 moles of H2O2 -----> 2 moles of H2O(l) + O2(g)

Solution Preview

P = 715 torr = 715*133 = 95095 Pa
T = 21 degC = 273+21 = 294 K
R = 8.31 J/mol/K
V = 3.31 L = 3.31*10^(-3) ...

Solution Summary

This solution includes three detailed steps of calculations.

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