Question

Choose the correct answer :

1. Production of iron in blast furnace follows the following equation

Fe3O4(s)+4CO(g)→3Fe(I)+4CO22(g)

when 4.640 kg of Fe₃O₄ and 2.520 kg of CO are allowed to react then the amount of iron (in g) produced is

[Given : Molar Atomic mass (g mol^–1) : Fe = 56

Molar Atomic mass (g mol^–1) : O = 16

Molar Atomic mass (g mol^–1) : C = 12]

• A. 1400
• B. 2200
• C. 3360
• D. 4200

Answer 1

The Correct Option is C

To find the amount of iron produced in the given reaction when 4.640 kg of Fe₃O₄ and 2.520 kg of CO are reacted, we will follow these steps:

1. First, determine the molar mass of Fe₃O₄ using the given atomic masses:
   • Fe: 56 g/mol
   • O: 16 g/mol
   The molar mass of Fe₃O₄ is calculated as follows: 3 \times 56 + 4 \times 16 = 168 + 64 = 232 \text{ g/mol}
2. Convert the mass of Fe₃O₄ to moles: \text{Moles of Fe}_3\text{O}_4 = \frac{4640}{232} = 20 \text{ moles}
3. Similarly, determine the molar mass of CO:
   • C: 12 g/mol
   • O: 16 g/mol
   The molar mass of CO is: 12 + 16 = 28 \text{ g/mol}
4. Convert the mass of CO to moles: \text{Moles of CO} = \frac{2520}{28} = 90 \text{ moles}
5. According to the balanced reaction: \text{Fe}_3\text{O}_4(s) + 4\text{CO}(g) \rightarrow 3\text{Fe}(l) + 4\text{CO}_2(g) 1 mole of Fe₃O₄ reacts with 4 moles of CO to produce 3 moles of Fe.
6. Determine the limiting reagent:
   • Fe₃O₄: 20 moles available, needs 20 × 4 = 80 moles of CO
   • CO: 90 moles available
   Fe₃O₄ is the limiting reagent since it would fully react with 80 moles of CO, leaving CO in excess.
7. From the stoichiometry, 1 mole of Fe₃O₄ produces 3 moles of Fe: 20 \times 3 = 60 \text{ moles of Fe}
8. Calculate the mass of iron produced: \text{Mass of Fe} = 60 \times 56 = 3360 \text{ g}

Therefore, the amount of iron produced is 3360 g.