The combustion of 0.4196 g of a hydrocarbon releases 17.55 kJ of heat. The masses of the products formed, viz. CO2 and H2O are 1.419 g and 0.290 g, respectively. Calculate the empirical formula of the hydrocarbon and its standard enthalpy of formation assuming that its molar mass is 78 g.
The combustion of 0.4196 g of a hydrocarbon releases 17.55 kJ of heat. The masses of the products formed, viz. CO2 and H2O are 1.419 g and 0.290 g, respectively. Calculate the empirical formula of the hydrocarbon and its standard enthalpy of formation assuming that its molar mass is 78 g.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.106QE: A compound is 82.7% carbon and 17.3% hydrogen, and has a molar mass of approximately 60 g/mol. When...
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