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.)

FREE Expert Solution

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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