Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?
A)151 g
B)123 g
C)50.3 g
D)37.7 g
E)9.41 g

Question

Quizplus · Accepted Answer

The reaction between lead(II) sulfide (PbS) and hydrogen peroxide (H2O2) to form lead(II) sulfate (PbSO4) and water (H2O) can be represented by the balanced chemical equation: PbS + 4 H2O2 → PbSO4 + 4 H2O. To find the mass of H2O2 needed, we first calculate the moles of PbS using its molar mass (239.26 g/mol), then use the stoichiometry of the reaction to find the moles of H2O2 needed, and finally convert this to grams using the molar mass of H2O2 (34.01 g/mol).Moles of PbS = 265 g / 239.26 g/mol = 1.107 molesMoles of H2O2 needed = 1.107 moles PbS * 4 moles H2O2/mole PbS = 4.428 moles H2O2Mass of H2O2 needed = 4.428 moles * 34.01 g/mol = 150.6 g, which rounds to 151 g.

Lead(II) Sulfide Was Once Used in Glazing Earthenware