Solution Found!
Answer: The combustion of 0.4196 g of a hydrocarbon
Chapter 6, Problem 140P(choose chapter or problem)
The combustion of 0.4196 g of a hydrocarbon releases 17.55 kJ of heat. The masses of the products are \(\mathrm{CO}_{2}=1.419\ \mathrm{g}\) and \(\mathrm{H}_{2} \mathrm{O}=0.290\ \mathrm{g}\). (a) What is the empirical formula of the compound? (b) If the approximate molar mass of the compound is 76 g, calculate its standard enthalpy of formation.
Questions & Answers
QUESTION:
The combustion of 0.4196 g of a hydrocarbon releases 17.55 kJ of heat. The masses of the products are \(\mathrm{CO}_{2}=1.419\ \mathrm{g}\) and \(\mathrm{H}_{2} \mathrm{O}=0.290\ \mathrm{g}\). (a) What is the empirical formula of the compound? (b) If the approximate molar mass of the compound is 76 g, calculate its standard enthalpy of formation.
ANSWER:Step 1 of 3
(a)
From the given,
Mass of Carbon = 1.49 g
Mass of Hydrogen = 0.290 g
Mass of Hydrocarbon = 0.4196 g
Heat released = 17.55 KJ