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Answer: The combustion of 0.4196 g of a hydrocarbon

Chapter 6, Problem 140P

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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.

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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

 

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