Adiabatic Flame Temperature Calculation for Methane Combustion

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To calculate the adiabatic flame temperature for methane combustion, the reaction involves methane (CH4) reacting with oxygen (O2) from the air, while nitrogen (N2) and argon (Ar) act as inert components. The combustion reaction can be represented as CH4 + 2O2 → CO2 + 2H2O, assuming complete combustion. The volume of air used is 11.264, which contains 21% O2, necessary for the reaction. It is important to note that nitrogen and argon do not participate in the reaction but must be accounted for in the energy balance. Assumptions made include ideal gas behavior and complete combustion conditions.
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One volume of CH4 is mixed with V volumes of air (78 vol.% N2,21 vol.% O2,1 vol.% Ar) at 1 atm and 25°C; then the mixture is ignited. Find the temperature of adiabatic combustion (the adiabatic flame temperature). The volume of air is 11.264.

Explicitly list any assumptions you made while working on this problem.

I don't really know how to write the reaction of CH4 with the air, if anybody could give any insight on this question that'd be so helpful.
 
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There is no such thing as reaction of methane with the air. It will react with oxygen only. Both nitrogen and argon will just be there (and they have to be heated).
 

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