Question

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One of the components that make up common table sugar is fructose, a compound that contains only carbon, hydrogen, and oxygen. Complete combustion of 1.50 g of fructose produced 2.20 g of carbon dioxide and 0.900 g of water. What is the empirical formula of fructose?

Answer 1

Mass of fructose = 1.50 g mass of co_2 = 2.20 g molar mass of co_2 = 44 g/mol 44 g co_2 contains 12 g c 2.20 g co_2 contains 12/44 times 2.20 g c = 0.6 g carbon mass of carbon = 0.6g mass of h_2 o = 0.9 g molar mass of h_2 o = 18 g/mol 18 g h_2 o contains 2 g h ag h_2 o contains 2/18 times .9 = 0.1 g h mass of h = 0.1 g mass of o = mass of structure - (mass of c, h) mass of o = 1.5 - (0.6 + 0.1)g mole of o = 0.8 g mole of c = mass of c/12 = .6/12 = 0.05 moles mole of h = mass of h/1 = .1/1 = .1 moles moles of o = mass of o/16 = 8/16 = 0.05 mole \r\n moles of c h o 0.5: .1: .0.5 5: 10: 5 1: 2: 1 c_1 h_2 o_1 empirical formula = ch_2 o