1.) When 3.065 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 9.616 grams of CO2 and 3.937 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 70.13 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
1.) When 3.065 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 9.616 grams of CO2 and 3.937 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 70.13 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
2.) When 3.774 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 12.76 grams of CO2 and 2.612 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found to be 26.04 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
3.) A 8.727 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 12.38 grams of CO2 and 7.601 grams of H2O are produced.
In a separate experiment, the molar mass is found to be 62.07 g/mol. Determine the empirical formula and the molecular formula of the organic compound.
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