Question

In: Chemistry

You are searching for an inexpensive synthetic route to make anthraquinone to use it as the...

You are searching for an inexpensive synthetic route to make anthraquinone to use it as the active component in a new laxative formulation. Reaction of benzene and phthalic anhydride yielded a yellow solid thought to be anthraquinone. Combustion analysis of 0.520 g of the yellow solid yielded 1.54 g of carbon dioxide and 0.180 g of water; (all carbon dioxide and water formed by combustion were isolated and weighed). In another experiment, the molar mass of the yellow solid was found to be approximately 205 g/mol. Use the analysis information above to determine the molecular formula of the yellow solid.

Solutions

Expert Solution

moles of CO2 = 1.54 / 44 = 0.035

moles of C = 0.035

mass of Carbon = 12 x 0.035 = 0.42 g

moles of H2O = 0.180 / 18 = 0.01

moles of H = 2 x 0.01 = 0.02

mass of hydroegen = 0.02 g

Oxygen mass = 0.520 - (0.42 + 0.02 ) = 0.08 g

moles of O = 0.08 /16 = 0.005

C                H              O

0.035      0.02        0.005

    7                4              1

C7H4O -----------------------> empirical formula

mass of empirical formula = 104 g

molar mass of yellow solid = 205 g

n = molar mass / emperical formula mass = 205 / 104

    = 2

molecular formula = 2 x C7H4O

molecular formula = C14H8O2


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