You burn 12.3 mL of octane (C8H18, a liquid with a density of 0.703 g/mL and...

You burn 12.3 mL of octane (C8H18, a liquid with a density of 0.703 g/mL and a molar mass of 114.23 g/mol, which is a major component of gasoline) in a piston. Initial conditions of the piston:

Initial volume of 1.6 L (ignore the small volume contribution of liquid octane).

Initial pressure of 1.00 atm (which is also this system’s ambient pressure).

Initial temperature of 0.00 °C (which is also this system’s ambient temperature).

Initial content is air, 20.0% O2 and 80.0% N2.

You then perform a complete combustion reaction (hydrocarbon reacting with molecular gaseous oxygen to yield carbon dioxide gas and water VAPOR gas).

Final conditions of the piston:

Final pressure of 1.00 atm (it was allowed to equilibrate to ambient pressure)

Final temperature of 0.00 °C (it was allowed to equilibrate to ambient temperature).

Final contents contains the combustion products, leftover oxygen (if any), and unreacted nitrogen.

Calculate the final volume of the piston

Expert Solution

Amanda K answered 7 months ago

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