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A 0.6996 g sample of a compound containing C, H, and F was burned to produce 0.6039 g CO2 and 0.1235 g H2O. If the molar mass of the compound was determined to be approximately 102.0 g/mol, what is its molecular formula?

  • chemistry -

    .6996g of sample at 102g/mol = 0.006859 mol

    .6039g CO2 at 44g/mol = 0.1373 mol of C
    .1235g H2O at 18g/mol = 0.006859 mol of H

    so, each mole of the compound produces 2 moles of H and 2 moles of C

    The formula is C2H2F?

    C2H2 has mass 26
    102-26 = 76
    Fluorine has mass 19
    76/19 = 4

    The compound has formula C2H2F4

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