When 4.6 g of matter is burned, 8.8 g of CO₂ and 5.4 g of H₂O are formed. The vapor density

| December 25, 2020 | education

When 4.6 g of matter is burned, 8.8 g of CO₂ and 5.4 g of H₂O are formed. The vapor density of this substance in the air is 1.59. Determine the molecular formula of this substance.

1) Let’s write the formula Cx Well Oz
2) It is necessary to find the amount of substances
V (CO2) = m / M = 8.8 / 44 = 0.2 mol
V (H2O) = m / M = 5.4 / 18 = 0.3 mol
3) It is necessary to find the number of elements
V (C) = V (CO2) = 0.2 mol
V (H) = 2 * V (H2O) = 2 * 0.3 = 0.6 mol
4) Looking for masses
m (C) = 12 * 0.2 = 2.4 g
m (H) = 1 * 0.6 = 0.6 g
m (O) = 4.6- (2.4 + 0.6) = 1.6 g
5) We are looking for the number of elements of hydrogen
V (O) = 1.6 / 16 = 0.1 mol
6) Find how the indices relate
x: y: z = 0.2: 0.6: 0.1 = 2: 6: 1
The simplest formula is C2H6O
M (C2H6O) = 46 g / mol
7) Comparison
Mist = Mprost = 46/46 = 1
Molecular Formula – C2H6O
Answer: C2H6O



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