Asked by Grace
2.4 of a compound of carbon, hydrogen and oxygen gave on combustion, 3.52g carbon dioxide and 1.44g of water. The elative atomic mass of the compound was found to be 6o. What are the masses of carbon, hydrogen and oxygen in 2.4 of the compound
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Assuming the sample mass is 2.4 g and the molecular mass is 60:
- Carbon: from CO2 (44 g CO2 contains 12 g C)
m(C) = 3.52 × (12/44) = 0.96 g
- Hydrogen: from H2O (18 g H2O contains 2 g H)
m(H) = 1.44 × (2/18) = 0.16 g
- Oxygen: remainder
m(O) = 2.4 − (0.96 + 0.16) = 1.28 g
Moles: C = 0.96/12 = 0.08; H = 0.16/1 = 0.16; O = 1.28/16 = 0.08 → ratio 1:2:1 → empirical formula CH2O (mass 30). With molar mass 60, molecular formula = C2H4O2.
- Carbon: from CO2 (44 g CO2 contains 12 g C)
m(C) = 3.52 × (12/44) = 0.96 g
- Hydrogen: from H2O (18 g H2O contains 2 g H)
m(H) = 1.44 × (2/18) = 0.16 g
- Oxygen: remainder
m(O) = 2.4 − (0.96 + 0.16) = 1.28 g
Moles: C = 0.96/12 = 0.08; H = 0.16/1 = 0.16; O = 1.28/16 = 0.08 → ratio 1:2:1 → empirical formula CH2O (mass 30). With molar mass 60, molecular formula = C2H4O2.
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