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7 February, 09:47

What mass of hydrogen peroxide should result when 1.50 g of barium peroxide is treated?

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  1. 7 February, 10:15
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    Barium peroxide is BaO2.

    Hydrogen peroxide is H2O2

    This reaction produces hydrogen peroxide from barium peroxide:

    BaO2 + H2SO4 - - - > BaSO4 + H2O2

    So, 1 mol of BaO2 produces 1 mol of H2O2.

    Convert 1.50 g of BaO2 to moles:

    moles = mass in grams / molar mass

    molar mass of BaO2 = 137g/mol + 2*16g/mol = 169 g/mol

    moles of BaO2 = 1.50g / 169 g/mol = 0.00888 moles

    Then, the same number, 0.00888, will be produced of H2O2.

    Now convert 0.00888 moles of H2O2 to mass in grams:

    mass in grams = number of moles * molar mass

    molar mass of H2O2 = 2 * 1 g/mol + 2 * 16 g/mol = 34 g/mol

    mass of H2O2 = 0.00888 moles * 34 g/mol = 0.30192 grams.

    Rounded to 3 significant figures = 0.302 grams.

    Answer: 0.302 grams
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