Question
In: Chemistry
An unidentified organic compound containing only C, H, and O was subjected to combustion analysis. When...
An unidentified organic compound containing only C, H, and O was subjected to combustion analysis. When 228.4 g of the substance burned in oxygen gas, 627.4 g of carbon dioxide and 171.2 g of water were collected. Determine the mass of carbon in the original sample and the empirical formula. Please also provide an brief explanation for this problem in sentences. Thanks in advance
Solutions
Expert Solution
moles of CO2 = mass / molar mass
= 627.4 / 44
= 14.26
moles of C = 14.26
mass of C =14.26 x 12 = 171.1 g
mass of C = 171.1 g
moles of H2O = 171.2 / 18 = 9.51
moles of H = 2 x 9.51 = 19.0
mass of H = 19.1 g
mass of O = 228.4 - (19.1 + 171.1) = 38.2 g
moles of O = 38.2 / 16 = 2.39
moles ratio : C:H:O = 14.26 : 19.1 : 2.39
= 6 : 8 : 1
empirical formula = C6 H8 O
queen_honey_blossom answered 1 year agoRelated Solutions
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