The combustion of 0.4196 g of hydrocarbon releases 17.55 kJ of heat. The masses of the...

The combustion of 0.4196 g of hydrocarbon releases 17.55 kJ of heat. The masses of the products are 1.418 g of carbon dioxide (CO₂) and 0.290 g of water (H₂O). The standard formation enthalpy for CO₂(g) and H₂O(l) are −393.5 kJ/mol and −285.8 kJ/mol, respectively.

(a) What is the empirical formula of the compound?

(b) If the approximate molar mass of the compound is 76 g/mol, calculate the standard enthalpy of formation.

Δ

H

o

f

=

kJ

mol

Expert Solution

queen_honey_blossom answered 1 year ago

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The combustion of 0.4196 g of hydrocarbon releases 17.55 kJ of heat. The masses of the...

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