I have a natural gas combustion in pure oxygen related query,
CH4 + 2 O2 = CO2 + 2 H2O + heat
The Heat of combustion is for CH4 is ΔHc = 802.3 KJ/mol, for complete combustion of methane.
Now, the natural gas is coming at a certain mass flow rate (Kg/hr), which I can convert to mol/hr by dividing the flow rate with Molar mass of methane (g/mol). The number of moles per hour (mol/hr) can be multiplied to determine the Heat generated (KJ/hr) or released upon the reacting with pure Oxygen.
The question is, Am i doing it right ? Also, How does flow rate (quantity) of oxygen supplied for combustion influence the heat released. In other words how do I account for Oxygen as it does not have a calorific value (not a fuel) ?
Will appreciate your response,