To produce iron from iron ore (Fe2O3), you have to remove oxygen using the following chemical...

  

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To produce iron from iron ore (Fe2O3), you have to remove oxygen using the following chemical reaction, which produces CO: 2 FeO3 + 3 C 4 Fe + 3 CO In this question, you will simplify this process as the schematic diagram below and look at how much CO we emit per unit mass of pure iron produced. Note that graphite only consists of C. Dry air mol m = 100,300 K, 100 kPa Iron ore (Fe03) + Graphite (C), 2:3 by mole ratio mol m = 5,300 K Air+CO mixture through chimney at 1800 K Pure (Fe) at 1800 K Qcv =? Just like the first assignment, take air as a mixture of 78% N and 22% O by moles in the incoming air stream. Note that the composition of exiting gas mixture will be N, O, and CO. The heat capacities are Cre0,= 0.650- Cre = 0.451 Cgraphite=0.720; Assume these remain constant. The molar masses are Me0s= 160,Mee = 56, Mg graphite 12 Use (A.7/8/9) for all others. kg-K kg-k = Fe mol mol mol (a) Balance the following chemical equation on the right side [1 Pt]. (b) Determine the mass fractions of the exiting gas mixture [3 Pts]. (c) How much heat do you have to supply during this process per one ton of pure iron produced? Use absolute zero as the reference [8 Pts]. (d) How much kg of CO do you have to emit per one ton of pure iron produced? [2 Pts] (e) What is the exiting pressure of gas mixture? Assume the volume occupied by the gas mixture remain the same [4 Pts]. 78 N + 22 0 +2 FeO3 + 3 C Fe + N +0 + CO (f) Qualitatively explain what will happen to the exiting gas mixture composition if you decrease the mass fraction of graphite in the injection of iron ores. [2 Pts] *Note that the given process is highly simplified to fit the scope of this course. In reality, you have to leave some carbon in steel for strength toughness, and the source of carbon is coal, not graphite. Therefore, the byproducts from actual steal manufacturing are a lot 'dirtier than what is shown in this question. To produce iron from iron ore (FeO3), you have to remove oxygen using the following chemical reaction, which produces CO: 2 FeO3 +3C 4 Fe + 3 CO In this question, you will simplify this process as the schematic diagram below and look at how much CO we emit per unit mass of pure iron produced. Note that graphite only consists of C. Dry air m = 100- mol ,300 K, 100 kPa Iron ore (Fe0) + Graphite (C), 2:3 by mole ratio mol m=5,300 K Boss Qcv = ? Just like the first assignment, take air as a mixture of 78% N and 22% O by moles in the incoming air stream. Note that the composition of exiting gas mixture will be N, O, and CO. The heat capacities are Cre0, = 0.650- The molar masses are Mpes0=160 Air+CO mixture through chimney at 1800 K kg-K' Cre= 0.451- Mpe = 56, Mar mol kg-K Fe Pure (Fe) at 1800 K Cgraphite=0.720- Assume these remain constant. graphite 12 Use (A.7/8/9) for all others. kg.K mol To produce iron from iron ore (Fe2O3), you have to remove oxygen using the following chemical reaction, which produces CO: 2 FeO3 + 3 C 4 Fe + 3 CO In this question, you will simplify this process as the schematic diagram below and look at how much CO we emit per unit mass of pure iron produced. Note that graphite only consists of C. Dry air mol m = 100,300 K, 100 kPa Iron ore (Fe03) + Graphite (C), 2:3 by mole ratio mol m = 5,300 K Air+CO mixture through chimney at 1800 K Pure (Fe) at 1800 K Qcv =? Just like the first assignment, take air as a mixture of 78% N and 22% O by moles in the incoming air stream. Note that the composition of exiting gas mixture will be N, O, and CO. The heat capacities are Cre0,= 0.650- Cre = 0.451 Cgraphite=0.720; Assume these remain constant. The molar masses are Me0s= 160,Mee = 56, Mg graphite 12 Use (A.7/8/9) for all others. kg-K kg-k = Fe mol mol mol (a) Balance the following chemical equation on the right side [1 Pt]. (b) Determine the mass fractions of the exiting gas mixture [3 Pts]. (c) How much heat do you have to supply during this process per one ton of pure iron produced? Use absolute zero as the reference [8 Pts]. (d) How much kg of CO do you have to emit per one ton of pure iron produced? [2 Pts] (e) What is the exiting pressure of gas mixture? Assume the volume occupied by the gas mixture remain the same [4 Pts]. 78 N + 22 0 +2 FeO3 + 3 C Fe + N +0 + CO (f) Qualitatively explain what will happen to the exiting gas mixture composition if you decrease the mass fraction of graphite in the injection of iron ores. [2 Pts] *Note that the given process is highly simplified to fit the scope of this course. In reality, you have to leave some carbon in steel for strength toughness, and the source of carbon is coal, not graphite. Therefore, the byproducts from actual steal manufacturing are a lot 'dirtier than what is shown in this question. To produce iron from iron ore (FeO3), you have to remove oxygen using the following chemical reaction, which produces CO: 2 FeO3 +3C 4 Fe + 3 CO In this question, you will simplify this process as the schematic diagram below and look at how much CO we emit per unit mass of pure iron produced. Note that graphite only consists of C. Dry air m = 100- mol ,300 K, 100 kPa Iron ore (Fe0) + Graphite (C), 2:3 by mole ratio mol m=5,300 K Boss Qcv = ? Just like the first assignment, take air as a mixture of 78% N and 22% O by moles in the incoming air stream. Note that the composition of exiting gas mixture will be N, O, and CO. The heat capacities are Cre0, = 0.650- The molar masses are Mpes0=160 Air+CO mixture through chimney at 1800 K kg-K' Cre= 0.451- Mpe = 56, Mar mol kg-K Fe Pure (Fe) at 1800 K Cgraphite=0.720- Assume these remain constant. graphite 12 Use (A.7/8/9) for all others. kg.K mol