Oxygenated hydrocarbons (Oxy-HCs) are hydrocarbons that contain oxygenated functional groups, such as carbonylic (-CO-) and alcoholic (-OH) groups. Oxy-HCR can definitely be a potentially cleaner and renewable alternative to existing fossil. What is the total number of moles for the molecule and oxygen in 102.3 g of C4H8O3: Please show all your detailed calculations using your handwriting

Oxygenated hydrocarbons (Oxy-HCs) are hydrocarbons that contain oxygenated functional groups, such as carbonylic (-CO-) and alcoholic (-OH) groups. Oxy-HCR can definitely be a potentially cleaner and renewable alternative to existing fossil. What is the total number of moles for the molecule and oxygen in 102.3 g of C4H8O3: Please show all your detailed calculations using your handwriting

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 52E: Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00...

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In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
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