Problem: A gaseous fuel mixture contains 23.1% methane (CH4), 41.1% ethane (C2H6) and the rest propane (C3H8) by volume.When the fuel mixture contained in a 1.53 L tank, stored at 751 mmHg and 298 K, undergoes complete combustion, how much heat is emitted? (Assume that the water produced by the combustion is in the gaseous state.)

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We are asked how much heat is emitted


Since the gas are under the same conditions, the volume percent is the same as the mole percent. 


Calculate total moles: 

PV= nRTn = PVRTn = (751 mmHg×1 atm760  mmHg)(1.53 L)(0.08206  L- atmmol-K)(298 K)

n = 0.0617 mol


Calculate moles of each: 

mol CH4 = 0.231(0.0617 mol) = 0.014 mol CH4 mol C2H6 =0.411(0.0617 mol) = 0.025 mol C2H6 mol C3H8 =(1-0.231-0.411)(0.0617 mol) = 0.022 mol C3H8


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Problem Details

A gaseous fuel mixture contains 23.1% methane (CH4), 41.1% ethane (C2H6) and the rest propane (C3H8) by volume.

When the fuel mixture contained in a 1.53 L tank, stored at 751 mmHg and 298 K, undergoes complete combustion, how much heat is emitted? (Assume that the water produced by the combustion is in the gaseous state.)

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