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When 2.56 g of a compound containing only carbon, hydrogen, and oxygen is burned completely, 5.82 g of CO2 and 2.38 g of H2O are produced..?
What is the empirical formula of the compound? please also explain how. Thanks!
1 Answer
- FernLv 76 years agoFavorite Answer
5.82 g CO2 x 1 mole CO2/44 g CO2 x 1 mole C/ 1 mole CO2 = 0.132 moles C
2.38 g H2O x 1mole H2O/18 x 2 moles H/1mole H2O = 0.264 moles H
To obtain the weight of oxygen in the compound:
0.132 moles C x 12 g C / 1 mole C = 1.58g C
0.264 moles H x 1 g H/1mole H = 0.264 g H
Weight of oxygen:
2.56 g compound – 1.58 g C – 0.264 g H – 0.716 g O
0.716 g O x 1 mole O/ 16 g O = 0.0447 moles O
C0.132H0.264O 0.0447
Divide all moles by 0.0447
C2.95H5.9O1.0
Empirical Formula is: C3H6O