A XX-g sample of methane, CH4, is mixed with YY atm of O2 (an excess) in a VV L combustion chamber at 125.0°C. The combustion reaction to CO2 and H2O is initiated and the vessel is cooled back to 125.0°C. What is the final pressure in the combustion chamber assuming the reaction goes to completion?
CH4 + 2O2 ==> CO2 + 2H2O
3 mols of gas on the left goes to 3 mols of gas on the right.
Final pressure = initial pressure.
Initial pressure = pO2 + pCH4:
O2 = YY atm
CH4 = XXg x (1 mol/16 g) x (RT)/VV L
Check my thinking.
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