When 43.2 g of hydrocarbon was burned, 132 g of carbon dioxide and 64.8 g of water were formed.
| December 10, 2020 | education
When 43.2 g of hydrocarbon was burned, 132 g of carbon dioxide and 64.8 g of water were formed. Find the molecular formula of a given hydrocarbon if its oxygen density is 2.25.
n (C) = 132/44 = 3 mol
n (H) = 64.8 / 18 * 2 = 7.2 mol
M = 32 * 2.25 = 72 g / mol
n (C): n (H) = 3: 7.2 = 30: 72 = 5:12
the desired hydrocarbon – pentane c5h12
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