What mass of iron metal can be obtained from the reaction of 45.6kg Iron (III) oxide Fe3O4 with carbon monoxide CO as given in the following equation?
Fe3O4 + 4CO = 3Fe + 4CO2
To determine the mass of iron metal that can be obtained from the reaction, we need to use stoichiometry. Stoichiometry is the calculation of the quantitative relationships between reactants and products in a chemical reaction.
Step 1: Write down the balanced equation:
Fe3O4 + 4CO = 3Fe + 4CO2
Step 2: Calculate the molar mass of the substances involved:
- Iron (III) oxide (Fe3O4) has a molar mass of (55.85*3 + 16*4) = 231.52 g/mol.
- Carbon monoxide (CO) has a molar mass of (12.01 + 16.00) = 28.01 g/mol.
- Iron (Fe) has a molar mass of 55.85 g/mol.
Step 3: Convert the given mass of iron (III) oxide to moles:
Given mass of Fe3O4 = 45.6 kg = 45,600 g
Number of moles of Fe3O4 = Given mass / Molar mass
= 45,600 g / 231.52 g/mol
≈ 197.16 mol
Step 4: Determine the stoichiometric ratios between the substances in the balanced equation:
From the equation, we see that 1 mole of Fe3O4 reacts to form 3 moles of Fe.
Step 5: Calculate the moles of Fe that can be obtained:
Number of moles of Fe = Number of moles of Fe3O4 × (3 moles Fe / 1 mole Fe3O4)
= 197.16 mol × (3/1)
≈ 591.48 mol
Step 6: Convert moles of Fe to mass:
Mass of Fe = Number of moles of Fe × Molar mass of Fe
= 591.48 mol × 55.85 g/mol
≈ 33,022.38 g
≈ 33.022 kg
Therefore, the mass of iron metal that can be obtained from the reaction is approximately 33.022 kg.