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Methane gas (CH4) at -10°C is burned with pure O2 at 5°C. The O2 is fed...

Methane gas (CH4) at -10°C is burned with pure O2 at 5°C. The O2 is fed at a mol ratio of 1.8:1 relative to CH4. The flue gases leave at 90°C. All compounds exit in the gas phase. Assume the system is at steady state and no work is done. DHo f, CH4, gas = -74.84 kJ/mol Cp (for all gases and vapors): 30 J/mol.K DHo f, CO2, gas = -393.51 kJ/mol DHo f, H2O, gas = -241.83 kJ/mol a) What is the limiting reactant? b) Calculate the heat released per mol of O2 c) What would happen to the heat released per mol of O2 if we did the following: i) Increase temperature of reactants ii) Increase temperature of products iii) Increase feed ratio to 2 mol O2 : 1 mol CH4

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Amanda K answered 5 months ago
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