Problem: Some automobiles and buses have been equipped to burn propane (C3H8). Compare the amounts of energy that can be obtained per gram of C3H8(g) and per gram of gasoline, assuming that gasoline is pure octane, C8H18(l). (See Example 7‑11.) Look up the boiling point of propane. What disadvantages are there to using propane instead of gasoline as a fuel?

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Recall: The enthalpy of reaction (ΔH˚rxn) can be calculated from the reactants' and products' enthalpy of formation (∆H˚f) using the equation:

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Some automobiles and buses have been equipped to burn propane (C3H8). Compare the amounts of energy that can be obtained per gram of C3H8(g) and per gram of gasoline, assuming that gasoline is pure octane, C8H18(l). (See Example 7‑11.) Look up the boiling point of propane. What disadvantages are there to using propane instead of gasoline as a fuel?

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Our tutors have indicated that to solve this problem you will need to apply the Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.

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Based on our data, we think this problem is relevant for Professor McCamant's class at UR.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.