Enthalpies of combustion of , and are -890, -1411 and -1560 kJ/mole, respectively. Which has the highest fuel value (heat produced per gram of the fuel)?

Question

Enthalpies of combustion of $CH_4$, $C_2H_4$ and $C_2H_6$ are -890, -1411 and -1560 kJ/mole, respectively. Which has the highest fuel value (heat produced per gram of the fuel)?

Prashant Kotian · Accepted Answer

Correct answer: A. Fuel value is heat produced per gram. (molar mass = 16 g/mol): 890 / 16 = 55.6 kJ/g. (molar mass = 28 g/mol): 1411 / 28 = 50.4 kJ/g. (molar mass = 30 g/mol): 1560 / 30 = 52.0 kJ/g. Thus, has the highest fuel value.

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