Question

A gas mixture containing 50 g of Helium (He), 120 g of Argon (Ar), and 0.1 g Carbon monoxide (CO), has a total pressure of 2560 mbar. (M _Ar = 39.95 g/mol, M _He = 4 g/mol, M _CO = 28 g/mol)

The gas mixture is used to reduce hematite (Fe₂O₃, M = 159.6 g/mol) to iron. State which of the gas constituents is expected to react with hematite, derive a chemical equation for this reaction, and determine the mol fraction of gas mixture required for the reduction of 500 g hematite.                                             The hematite reduction is most efficient in the temperature range of 800 °C – 900 °C. Determine the temperature of the gas mixture, if the total volume of the reaction vessel is 0.5 m³, and ideal gas law relationships are assumed. State how the optimum operation temperature can be achieved. (p V = n R T; R = 8.314 J/mol K)       
The environmental conditions used for the hematite reduction may cause carburization of the reaction vessel, due to the decomposition of carbon monoxide into carbon (“Boudouard reaction”). Derive the thermodynamic equilibrium equation that gives the relationship of the carbon activity (a_c) as a function of the partial pressure of reaction gases.

Answer 1

Solukion- rom a ven Hekum olecular Helium Ne 4 on 20 פ3.00375 3a.aS 0. Qg tal Pressure (pt). 2sco "bar and So, cSSur He moles o Clium Lotal moles

(2 O B060 0.131 Co 0-003s CO 3003s 12-S+O-003 So, ta ressure o асн on resSure o ritu re e 2068.36 mbar He

-or Aron Co lcabon monoide) O. s693 mbar 64a Co equired 84 263, Is? # -4 mole Co veguired

acion S.S036 V- D.sm3 -S-34 丁 Co SS bar 820 c