Question

In ironmaking, iron metal can be separated from iron ore (Fe2O3) by heating the ore in a blast furnace in the presence of coke, which is a form of carbon: 2 Fe2O3(s) + 3 C(s) → 4 Fe(s) + 3 CO2(g) If 1000 kg of iron ore and 120 kg of coke are heated in a blast furnace, determine the limiting reactant, the theoretical yield of iron metal, and the theoretical yield of carbon dioxide.

Answer 1

The limiting reactant is iron ore, the theoretical yield of iron metal is 701.344 kg, and the theoretical yield of carbon dioxide is 413.292 kg.

Stoichiometric problem

From the equation of the reaction:

$2 Fe_2O_3(s) + 3 C(s) --- > 4 Fe(s) + 3 CO_2(g)$

The mole ratio of iron ore to carbon is 2:3.

Mole of 1000 kg of iron ore = 1000000/159.69

                                          = 6,262 moles

Mole of 120 kg carbon = 120000/12

                                 = 10,000 moles

Thus, it appears that the carbon is in excess while the iron ore is limited in availability.

The mole ratio of the iron ore and the iron produced is 1:2. Thus, the equivalent number of moles of iron produced will be:

              6,262 x 2 = 12,524 moles

Mass of 12,524 moles of iron = 12,524 x 56

                                                = 701,344 g or 701.344 kg

Thus, the theoretical yield of iron is 701.344 kg.

The mole ratio of the iron ore and the carbon dioxide produced is 2:3. The equivalent mole of carbon dioxide produced will be:

         6,262 x 3/2 = 9,393 moles

Mass of 9,393 moles carbon dioxide = 9,393 x 44

                                                         = 413,292 or 413.292 kg

The theoretical yield of carbon dioxide is, therefore, 413.292 kg.

More on stoichiometric problems can be found here: brainly.com/question/14465605

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