At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8915-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22°C and a pressure of 734 torr. Calculate the mass percent of NaClO3 in the original sample. (At 22°C the vapor pressure of water is 19.8 torr.)

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  1. 2NaClO3 ==> 2NaCl + 3O2
    Solve for mols O2.
    P gas (O2 + H2O) = 734 mm
    PH2O = 19.8
    PO2 = 734-19.8 = 714.2 mm
    Use PV = nRT and solve for n
    Convert to mols NaClO3 using the coefficients in the balanced equation.
    mols O2 x (2 mols NaClO3/3 mols O2) = ?
    Convert mols NaClO3 to grams. g = mols x molar mass.
    %NaClO3 = (g NaClO3/mass sample)*100 = ?

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