A gaseous fuel mixture contains 25.3% methane (CH4), 38.2% ethane (C2H6), and th

Question

A gaseous fuel mixture contains 25.3% methane (CH4), 38.2% ethane (C2H6), and the rest propane (C3H8)by volume.

When the fuel mixture contained in a 1.61 L tank, stored at 760 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.)

A gaseous fuel mixture contains 25.3% methane (CH4), 38.2% ethane (C2H6), and the rest propane (C3H8)by volume.

When the fuel mixture contained in a 1.61 L tank, stored at 760 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.)

Explanation / Answer

A gaseous fuel mixture contains 25.3% methane (CH4), 38.2% ethane (C2H6), and the rest propane (100-25.3-38.2= 36.5 %) (C3H8)by volume.

When the fuel mixture contained in a 1.61 L tank, stored at 760 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.)

mol gas = ideal gas law

PV = nRT

n = PV/(RT) = 760*1.61 / (62.4*298) =0.065801 mol

then

methane = 0.065801*25.3/100 = 0.0166476

ethane = 0.065801*38.2/100 = 0.02513

ethane = 0.065801*36.5/100 = 0.0240

HRxn:

methane = 889 kJ/mol

ethane = 1560 kJ/mol

propane = 2220 kJ/mol

then..

total heat = n of i *Hrxn of i

total heat =0.0166476*889 + 0.02513*1560 +0.0240*2220

total heat = 107.282kJ

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