The combustion yields the products, CO2 and H2O. Since all of the carbon in the unknown compound will go to CO2, we can calculate the amount of carbon in the 2.5g sample:
m(Carbon) = 12/44 * 2.5 = 0.6818g
Since all of the hydrogen in the unknown compound will go to H2O, we can calculate the amount of hydrogen in the 2.5g sample: m(Hydrogen) = 1.01/18.02 * 2.5 = 0.1401g Therefore, the mass of Oxygen in the sample must be equal to 2.5 - 0.6818 - 0.1401 = 1.6781g. Now to calculate mole ratios:
Carbon : 0.6818/12 = 0.05682 Hydrogen: 0.1401/1.01 =0.1387 Oxygen: 1.6781/16 = 0.10488 Dividing each by 0.05682, ration is C:H:O = 1: 2.44: 2 which is approx 1:2.5:2 So empirical formula is C2H5O4
Oct 2nd, 2014
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