Asked Feb 5, 2020

A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields 15.92 CO2 mg and 4.89 H2O mg . The molar mass of the compound is 118.1 g/mol. What are the empirical and molecular formulas of the compound?


Expert Answer

Step 1

The number of moles of the compound can be calculated by dividing the given mass of the compound by its molar mass. The molar mass of the compound is 118.1 gmol-1. Since 1g is equal to 1000 mg, 118.1 gmol-1 can be written as 118100 mgmol-1. The number of moles of the compound can be calculated as follows-

Chemistry homework question answer, step 1, image 1
Step 2

The number of moles of carbon dioxide and water can be calculated by dividing their given masses by their respective molar masses. The molar mass of carbon dioxide is 44000 mg and the molar mass of water is 18000 mg. The molar masses have been calculated as follows-

Chemistry homework question answer, step 2, image 1
Step 3

Let the number of carbon, hydrogen and oxygen atoms in one molecule of the compound be x, y and z respectively. On complete combustion of one mole of the organic compound, x moles of carbon dioxide and 0.5y moles of water vapor are produced. Since 9.04×10-5 moles of the compound produces 3....

Chemistry homework question answer, step 3, image 1

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