When a hydrocarbon weighing 6.4 g was burned, 19.8 g of carbon dioxide and 9 g of water were formed.
When a hydrocarbon weighing 6.4 g was burned, 19.8 g of carbon dioxide and 9 g of water were formed. The relative density of a substance for oxygen is 4. Find the molecular formula.
1. Let us write down the equation of combustion of an unknown hydrocarbon:
CxHy + O2 → xCO2 + 0.5yH2O;
2.Calculate the chemical amount of the generated carbon dioxide:
n (CO2) = m (CO2): M (CO2);
M (CO2) = 12 + 16 * 2 = 44 g / mol;
n (CO2) = 19.8: 44 = 0.45 mol;
3.Let us write down the formula of carbon dioxide according to its composition:
CO2 → C + 2O;
4.determine the amount of carbon:
n (C) = n (CO2) = 0.45 mol;
5.Calculate the chemical amount of the resulting water:
n (H2O) = m (H2O): M (H2O) = 9: 18 = 0.5 mol;
6.Set the amount of hydrogen:
H2O → 2H + O;
n (H) = n (H2O) * 2 = 0.5 * 2 = 1 mol;
7.determine the ratio of carbon to hydrogen in a hydrocarbon molecule:
n (C): n (H) = 0.45: 1 = 1: 2.2222, that is, the empirical formula CH2.2222;
8.Calculate the relative molecular weight of the hydrocarbon:
Mr (CxHy) = DO2 (CxHy) * Mr (O2) = 4 * 32 = 128;
9.Let’s find the ratio of the molecular weight of the hydrocarbon to the molecular weight of the empirical formula:
Mr (CH2.2222) = 12 + 2.2222 = 14.2222;
Mr (CxHy): Mr (CH2.2222) = 128: 14.2222 = 9,
10. Having increased the indices of the empirical formula by 9 times, we write down the molecular formula of the hydrocarbon:
C1 * 9 H2.2222 * 9 = C9H20.
Answer: С9Н20.