- #1

Tommybc

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1 kmol of gaseous methane (CH 4) is mixed with the correct amount of air in a closed vessel. The pressure and temperature of the mixture are 1 bar and 298 K respectively. The mixture is ignited. Estimate the adiabatic temperature of combustion.

Answer: ~2743 K

OK, so first I acquired the combustion equation and found the number of moles for stoichmetric conditions.

CH4 + x[O

_{2}+ (79/21)N

_{2}] → ACO

_{2}+ BH

_{2}O +CN

_{2}

Here by balancing the equation, I found that

CH4 + 2[O

_{2}+ (79/21)N

_{2}] → CO

_{2}+ 2H

_{2}O +7.5N

_{2}

Now I have a reference temperature, 298K which conveniently is 25° at 1 bar. This reads well with my steam table book for the products and reactants.

Considering Enthalpy of reactants: ΔH

_{0}=ΔU

_{0}+pdv=∑m

_{i}c

_{p}(T

_{0}-T

_{ref})

I can find the mass of constitutes but what about the enthalpys? At the referenced temperature I find Methane, O2 and N2 to be zero which makes the equation unsolvable. Could anyone point me in the right direction at least giving me the correct steps for this.

Many thanks

Tom